45
Solutions Unit Honors Chemistry
Solutions Unit
Honors Chemistry
Solutionbull Definition a homogeneous mixture of 2 or
more substances in a single physical statebull Parts solute and solvent (usually water)bull Types ndash Physical states solid (alloys) liquid gasndash Miscible vs Immiscible
bull Miscible Liquids that dissolve freely in one another in any proportion
bull Immiscible Liquid solutes and solvents that are not soluble
ndash Saturated Unsaturated and Supersaturatedndash Dilute vs Concentratedndash Electrolyte vs Nonelectrolyte
bull Saturated ndash soln containing the max amt of solute
bull Unsaturated ndash soln containing less solute than a sat soln under the existing conditions
bull Supersaturated ndash contains more dissolved solute than a saturated solution under the same conditions
Solubility Curves
supersaturated solution(stirred)
Supersaturated Solution of Sodium Thiosulfate
Solubility (physical change)
bull Definition mass of solute needed to make a saturated solution at a given temperaturendash solution equilibrium in
a closed systemndash dissolution harr
crystallizationndash Unit = g solute100 g
H2O
Solubility of solids in liquidsbull For most solids increasing
temperature increases solubilitybull In general ldquolike dissolves likerdquo
Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute
and solvent
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
Solu
bilit
y ( g
100
g w
ater
)
Saturated solrsquon
Supersaturated solution
Unsaturated solution
At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC
135 g100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC
unsaturatedWhat kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Solutionbull Definition a homogeneous mixture of 2 or
more substances in a single physical statebull Parts solute and solvent (usually water)bull Types ndash Physical states solid (alloys) liquid gasndash Miscible vs Immiscible
bull Miscible Liquids that dissolve freely in one another in any proportion
bull Immiscible Liquid solutes and solvents that are not soluble
ndash Saturated Unsaturated and Supersaturatedndash Dilute vs Concentratedndash Electrolyte vs Nonelectrolyte
bull Saturated ndash soln containing the max amt of solute
bull Unsaturated ndash soln containing less solute than a sat soln under the existing conditions
bull Supersaturated ndash contains more dissolved solute than a saturated solution under the same conditions
Solubility Curves
supersaturated solution(stirred)
Supersaturated Solution of Sodium Thiosulfate
Solubility (physical change)
bull Definition mass of solute needed to make a saturated solution at a given temperaturendash solution equilibrium in
a closed systemndash dissolution harr
crystallizationndash Unit = g solute100 g
H2O
Solubility of solids in liquidsbull For most solids increasing
temperature increases solubilitybull In general ldquolike dissolves likerdquo
Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute
and solvent
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
Solu
bilit
y ( g
100
g w
ater
)
Saturated solrsquon
Supersaturated solution
Unsaturated solution
At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC
135 g100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC
unsaturatedWhat kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
bull Saturated ndash soln containing the max amt of solute
bull Unsaturated ndash soln containing less solute than a sat soln under the existing conditions
bull Supersaturated ndash contains more dissolved solute than a saturated solution under the same conditions
Solubility Curves
supersaturated solution(stirred)
Supersaturated Solution of Sodium Thiosulfate
Solubility (physical change)
bull Definition mass of solute needed to make a saturated solution at a given temperaturendash solution equilibrium in
a closed systemndash dissolution harr
crystallizationndash Unit = g solute100 g
H2O
Solubility of solids in liquidsbull For most solids increasing
temperature increases solubilitybull In general ldquolike dissolves likerdquo
Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute
and solvent
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
Solu
bilit
y ( g
100
g w
ater
)
Saturated solrsquon
Supersaturated solution
Unsaturated solution
At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC
135 g100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC
unsaturatedWhat kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
supersaturated solution(stirred)
Supersaturated Solution of Sodium Thiosulfate
Solubility (physical change)
bull Definition mass of solute needed to make a saturated solution at a given temperaturendash solution equilibrium in
a closed systemndash dissolution harr
crystallizationndash Unit = g solute100 g
H2O
Solubility of solids in liquidsbull For most solids increasing
temperature increases solubilitybull In general ldquolike dissolves likerdquo
Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute
and solvent
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
Solu
bilit
y ( g
100
g w
ater
)
Saturated solrsquon
Supersaturated solution
Unsaturated solution
At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC
135 g100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC
unsaturatedWhat kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Solubility (physical change)
bull Definition mass of solute needed to make a saturated solution at a given temperaturendash solution equilibrium in
a closed systemndash dissolution harr
crystallizationndash Unit = g solute100 g
H2O
Solubility of solids in liquidsbull For most solids increasing
temperature increases solubilitybull In general ldquolike dissolves likerdquo
Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute
and solvent
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
Solu
bilit
y ( g
100
g w
ater
)
Saturated solrsquon
Supersaturated solution
Unsaturated solution
At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC
135 g100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC
unsaturatedWhat kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Solubility of solids in liquidsbull For most solids increasing
temperature increases solubilitybull In general ldquolike dissolves likerdquo
Depends onndash Type of bondingndash Polarity of moleculendash Intermolecular forces between solute
and solvent
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
Solu
bilit
y ( g
100
g w
ater
)
Saturated solrsquon
Supersaturated solution
Unsaturated solution
At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC
135 g100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC
unsaturatedWhat kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Solubility Graph for NaNO3
0
10
20
30
40
50
60
70
80
90
100
110
120
130
140
150
160
170
180
0 10 20 30 40 50 60 70 80 90 100 110
Temperature (deg C)
Solu
bilit
y ( g
100
g w
ater
)
Saturated solrsquon
Supersaturated solution
Unsaturated solution
At 20oC a saturated solution contains how many grams of NaNO3 in 100 g of waterWhat is the solubility at 70oC
135 g100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30oC
unsaturatedWhat kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Solubility of Gasesbull Gases are less
soluble at high temperatures than at low temperatures
bull Increasing temperature decreases solubility
bull Increasing pressure increases solubility
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
bull Increasing pressure increases solubilitybull The quantity of gas that dissolves in a
certain volume of liquid is directly proportional to the pressure of the gas (above the solution)
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
bull Effervescence ndash rapid escape of gas dissolved in liquid
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Factors Affecting Solubilitybull Increase surface area of solute
(crushing)bull Stirshakebull Increase temperature
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Dissolution Processbull Ionic Compounds
NaCl(s) Na+1(aq) + Cl-1(aq)
ndash For dissolution to occur must overcome solute attractions and solvent attractions
ndash Dissociation Reaction the separation of IONS when an ionic compound dissolves (ions already present)
ndash Try calcium chloride
hexahydrated for Na+1 most cations have 4-9 H2O molecules
6 is most common
Solvation process of solvent moleculessurrounding solute
Hydration solvation with water
nonelectrolyte
electrolyte
Dissolving NaCl in water
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Dissolution Processbull Molecular Compoundsndash Nonpolar molecular solids do not dissolve in
polar solvents bull naphthalene
ndash Polar moleculebull C12H22O11(s) C12H22O11(aq) bull Molecular solvationbull Nonelectrolyte
ndash Polar moleculebull HCl(g) H+1(aq) + Cl-1(aq) or bull HCl(g) + H2O H3O+1(aq) + Cl-1(aq)bull Ionization ions formed from solute molecules by
action of solvent (no ions initially present)bull Nonelectrolyte (HCl) electrolyte (ions)
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Electrolyte vs Nonelectrolyte
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Concentrationbull Percent concentration by mass (mass
ndash (solutesolution) x 100 = Concentrationbull Molarity (M)
ndash Moles of soluteLiters of solution = molLbull Molality (m)
ndash Moles of solutemass of solvent = molkgbull ppm and ppb
ndash Used for very dilute solutionsbull Dilution ndash a process in which more solvent is
added to a solutionndash How is this solution different
bull Volume color molarityndash How is it the same
bull Same mass of solute same moles of solutendash In Dilution ONLY ndash M1V1 = M2V2
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Net Ionic Equationsbull Net ionic equations are equations that show
only the soluble strong electrolytes reacting (these are represented as ions) and omit the spectator ions which go through the reaction unchangedndash Substances that are aqueous break down into ionsndash Substances that pure solids liquids or gases do
not break down in solution ndash Hint Remember to check solubility rules to
determine if a precipitate forms
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Energy Changesbull Heat of solution = Hsolnbull Endothermic
ndash Solute particles separating in solidndash Solvent particles moving apart to allow solute to enter
liquidndash Energy absorbed
bull Exothermicndash Solute particles separating in solidndash Solvent particles attracted to solvating solute particlesndash Energy released
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Colligative Propertiesbull Definition physical properties of
solutions that differ from properties of its solvent ndash Property depends upon the number of
solute particles in solutionbull Types
1 Vapor Pressure2 Boiling Point ELEVATION3 Freezing Point DEPRESSION
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Vapor PressureA measure of the tendency of molecules to escape from a liquid
bull For nonvolatile liquids or solid solutesbull A nonvolatile solute will typically increase the
boiling point and decrease the freezing point bull Adding a nonvolatile solute lowers the
concentration of water molecules at the surface of the liquid ndash This lowers the tendency of the water molecules to
leave the solution and enter the gas phase ndash Therefore the vapor pressure of the solution is LESS
than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor Pressure (kPa)
100
40
20
60
80
100H2O solution
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Boiling Point Elevationbull tb = boiling point elevationbull tb = iKbmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kb = molal bp elevation constantndash Kb = 0512degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash bp of solution = bp of solvent + tb
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Freezing Point Depressionwhen a solution freezes the solvent solidifies as a pure substance
deviates for more concentrated solutions
bull tf = freezing point depressionbull tf = iKfmndash i = molality conversion factor for ionic
compounds adjust for of ions actually present in solution (dissociation process)
ndash Kf = molal freezing point depression constantndash Kf = 1858degCkg H2O
moles of solute (ions or molecules)ndash m = molality = moles solute
kg of solventndash fp of solution = fp of solvent - tf
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Boiling Point Elevation and Freezing Point Problems
1 At what temperature will a solution begin to boil if it is composed of 150 g potassium nitrate in 350 g of waterndash Solute
2 At what temperature will a solution begin to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterndash Solute
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Naming Acids Review A Binary ndash H +one anion Prefix ldquohydrordquo+ anion name +ldquoicrdquoacid
Ex) HCl hydrochloric acidEx) H3P hydrophosphoric acid
B Tertiary ndash H + polyatomic anion no Prefix ldquohydrordquo
(oxo) end ldquoaterdquo = ldquoicrdquo acidend ldquoiterdquo = ldquoousrdquo acid
Ex) H2SO4 sulfuric acidEx) H2SO3 sulfurous acid
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Properties of Acids and Bases
Taste Touch Reactions with Metals
Electrical Conductivity
Acid sour
looks like water burns stings
Yes-produces
H2 gaselectrolyte in solution
Base(alkali) bitter
looks like water feels
slippery
No Reaction
electrolyte in solution
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Indicators Turn 1 color in an acid and another color in a base
A Litmus Paper Blue and RedAn aciD turns blue litmus paper reDA Base turns red litmus paper Blue
B Phenolphthalein colorless in an acid and pink in a base
C pH paper range of colors from acidic to basic
D pH meter measures the concentration of H+ in solution
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
bull Neutralization A reaction between an acid and base When an acid and base neutralize water and a salt (ionic solid) form
Acid + Base rarr Salt + Water
Ex) HCl + NaOH rarr NaCl + HOH
Reactions
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Arrhenius Definition (1884)A An acid dissociates in water to produce more
hydrogen ions H+HCl H+1 + Cl-1
B A base dissociates in water to produce more hydroxide ions OH-
NaOH Na+1 + OH-1
C Problems with Definitionbull Restricts acids and bases to water solutionsbull Oversimplifies what happens when acids
dissolve in waterbull Does not include certain compounds that have
characteristic properties of acids amp bases Ex) NH3 (ammonia) doesnrsquot fit
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Bronsted-Lowry Definition (1923)A An acid is a substance that can donate hydrogen ions
Ex) HCl rarr H+ + Cl-
ndash Hydrogen ion is the equivalent of a protonndash Acids are often called proton donorsndash Monoprotic (HCl) diprotic (H2SO4) triprotic (H3PO4)
B A base is a substance that can accept hydrogen ions Ex) NH3 + H+ rarr NH4
+
ndash Bases are often called proton acceptorsC Advantages of Bronsted-Lowry Definition
bullAcids and bases are defined independently of how they behave in water
bullFocuses solely on hydrogen ions
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Hydronium IonHydronium Ion ndash H3O+ This is a complex ion
that forms in water H+1 + H2O H3O+1
To more accurately portray the Bronsted-Lowry the hydronium ion is used instead of the hydrogen ion
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
STRONG AcidBase versus WEAK AcidBase
Strength refers to the of molecules that form IONS
A strong acid or base will completely ionize (gt95 as ions) This is represented by a single () arrow
HNO3 + H2O H3O+ + NO3-
A weak acid or base will partially ionize (lt5 as ions) This is represented by a double (harr) arrow
HOCl + H2O harr H3O+ + ClO-
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
HF lt HCl lt HBr lt HIincreasing strength
7 Strong AcidsHNO3 H2SO4 HClO3HClO4 HCl HBrHI
8 Strong BasesLiOH NaOH KOHRbOH CsOH Ca(OH)2Sr(OH)2 Ba(OH)2
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Strength vs Concentrationbull Strength refers to the percent of
molecules that form ions
bull Concentration refers to the amount of solute dissolved in a solvent Usually expressed in molarity
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Ionization of Acids amp Bases
bull H2SO4 2 H+ + SO4-2
ndash Sulfuric acid
bull H3PO3 ndash Phosphorous acid
bull Ca(OH)2 ndash Calcium hydroxide
3 H+ + PO3-3
Ca+2 + 2 OH-1
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Conjugate Acid-Base Pairs A pair of compounds that differ by only one hydrogen ion
A Acid donates a proton to become a conjugate base
B Base accepts proton to become a conjugate acid
bull A strong acid will have a weak conjugate base
bull A strong base will have a weak conjugate acid
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Acid (A) Base (B) Conjugate Acid (CA) Conjugate Base (CB)
NH3 + H2O harr NH4+ + OH-
HCl + H2O harr Cl- + H3O+
bull Base and Conjugate Acid are a Conjugate Pair
bull Acid and Conjugate Base are a Conjugate Pair
B
B
A
A
CA CB
CB CA
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
1 H2O + H2O harr H3O+ + OHminus B A CA CB
2 H2SO4 + OHminus harr HSO4minus + H2O
A B CB CA 3 HSO4
minus + H2O harr SO4minus2 + H3O+
A B CB CA4 OHminus + H3O+ harr H2O + H2O
B A CA CB
AciDonates amp Bases accept
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
The Self-ionization of Water amp pH1 Water is amphoteric it acts as both an acid and a base in the
same reactionEx) H2O(l) + H2O(l) harr H3O+
(aq) + OH-(aq)
Keq = equilibrium constant = [H3O+] [OH-]Because reactants and products are at equilibrium liquid water is
not included in the equilibrium expression
25C [H3O+] = 1 x 10-7 M and [OH-] = 1 x 10-7 M Kw = ion product constant or equilibrium constant for water
Kw = [H3O+] [OH-] = 1 x 10-14 M2 10 x 10-14 M2 = [10 x 10-7 M] [10x10-7 M]
10 x 10-14 = [H3O+] [OH-]
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Acids [H3O+] gt 1 x 10-7 MBases [OH-] gt 1 x 10-7 M
Using Kw in calculations If the concentration of H3O+ in the blood is 40 x 10-8 M what is the concentration of OH ions in the blood Is blood acidic basic or neutral
Kw = [H3O+] [OH-]10 x 10-14 M2 = [40 x 10-8 M] [OH-]
25 x 10-7 M = [OH-] slightly basic
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
The pH scale (1909) the power of HydrogenA Measure of H3O+ in solutionB pH = -log[H3O+]C Range of pH 0-14
pH lt 7 acidpH gt 7 basepH = 7 neutral
D pOH = -log[OH-]E pH + pOH = 14
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
H+
OH
-pH [H3O+] [OH-]14 1x10-14 1x100
13 1x10-13 1x10-1
12 1x10-12 1x10-2
11 1x10-11 1x10-3
10 1x10-10 1x10-4
9 1x10-9 1x10-5
8 1x10-8 1x10-6
7 1x10-7 1x10-7
6 1x10-6 1x10-8
5 1x10-5 1x10-9
4 1x10-4 1x10-10
3 1x10-3 1x10-11
2 1x10-2 1x10-12
1 1x10-1 1x10-131
14
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
Significant Digits Rulebull The number of digits AFTER
THE DECIMAL POINT in your answer should be equal to the number of significant digits in your original number
bull Ex -log[87x10-4M] ndashCalc Answer = 30604807474 ndashSig Fig pH = 306
