Chemical Foundations - California State University, Northridgejte35633/lectures/Chemis… · PPT...

SolutionsSolutionsChap. 15Chap. 15

I.I. What is a solution?What is a solution?

I.I. What is a solution?What is a solution?A.A. TermsTerms


1.1. Solute/solventSolute/solvent

The solute is the substance that gets .The solvent does the .


1.1. Solute/solventSolute/solvent

The solute is the substance that gets dissolved.The solvent does the dissolving.

solute

solvent


1.1. Solute/solventSolute/solvent2.2. Soluble/insolubleSoluble/insoluble

A substance that is can be dissolved.


1.1. Solute/solventSolute/solvent2.2. Soluble/insolubleSoluble/insoluble

A substance that is soluble can be dissolved.


1.1. Solute/solventSolute/solvent2.2. Soluble/insolubleSoluble/insoluble3.3. Miscible/ Miscible/

immiscibleimmiscible

Miscible substances are that will dissolve in each other.


1.1. Solute/solventSolute/solvent2.2. Soluble/insolubleSoluble/insoluble3.3. Miscible/ Miscible/

immiscibleimmiscible

Miscible substances are liquids that will dissolve in each other.


1.1. Solute/solventSolute/solvent2.2. Soluble/insolubleSoluble/insoluble3.3. Miscible/ immiscibleMiscible/ immiscible4.4. Electrolytes/non-Electrolytes/non-

electrolyteselectrolytes

Electrolytes are liquids that are capable of conducting electricity.

I.I. What is a solution?What is a solution?B.B. Types of solutionsTypes of solutions


1.1. Gaseous solutionsGaseous solutions

Air and other mixtures of gases


1.1. Gaseous solutionsGaseous solutions2.2. Liquid solutionsLiquid solutions

In some cases water is the solvent. These are called ( ).


1.1. Gaseous solutionsGaseous solutions2.2. Liquid solutionsLiquid solutions

In some cases water is the solvent. These are called (aqueous).


1.1. Gaseous solutionsGaseous solutions2.2. Liquid solutionsLiquid solutions3.3. Solid solutionsSolid solutions

Combinations of solids. Some are homogenous mixtures of metals ( )


1.1. Gaseous solutionsGaseous solutions2.2. Liquid solutionsLiquid solutions3.3. Solid solutionsSolid solutions

Combinations of solids. Some are homogenous mixtures of metals (alloys)

I.I. What is a solution?What is a solution?C.C. Making a solutionMaking a solution


1.1. Solute/solvent particles Solute/solvent particles are separated.are separated.



2.2. Solvent particles are Solvent particles are attracted to solute attracted to solute particles.particles.

This is called solvation.With the solvent this is called hydration




This is called solvation.With the solvent water this is called hydration




3.3. ‘‘Like dissolves like’Like dissolves like’

Polar/Non-polar SubstancesPolar/Non-polar Substances

Polar Non-polar

Water Carbon tetrachloride

Methanol Toluene (paint thinner)

Ethanol Hexane, heptane, octane

Acetic acid Benzene

Acetone Oil

Ionic compounds


1.1. Water is polar because it has Water is polar because it has two oppositely two oppositely ends ends

D.D. Dissolving Ionic Compounds Dissolving Ionic Compounds in Hin H22OO


1.1. Water is polar because it has Water is polar because it has two oppositely two oppositely chargedcharged ends ends




2.2. The The end of water is end of water is attracted to the anionattracted to the anion

Anion = negative ion




2.2. The The positivepositive end of water is end of water is attracted to the anionattracted to the anion

Anion = negative ion



3.3. The combined The combined of water of water molecules overcomes the molecules overcomes the attractive force of solute.attractive force of solute.



3.3. The combined The combined pullpull of water of water molecules overcomes the molecules overcomes the attractive force of solute.attractive force of solute.



3.3. The combined The combined pullpull of water of water molecules overcomes the molecules overcomes the attractive force of solute.attractive force of solute.

4.4. The ionic compound is The ionic compound is dissociated into individual dissociated into individual ions.ions.

Ex. NaCl (s) Na+ + Cl-


I.I. What is a solution?What is a solution?E.E. Dissolving Molecular Dissolving Molecular

Compounds in HCompounds in H22O.O.


1.1. Water’s charged ends are Water’s charged ends are attracted to charged attracted to charged portions of solute.portions of solute.

E.E. Dissolving Molecular Dissolving Molecular Compounds in HCompounds in H22O.O.



2.2. The solute is surrounded by The solute is surrounded by water molecules.water molecules.




2.2. The solute is surrounded by The solute is surrounded by water molecules.water molecules.

3.3. The solute remains intact.The solute remains intact.


I.I. What is a solution?What is a solution?F.F. Rate of SolvationRate of Solvation

To speed up solvation. . .To speed up solvation. . .


1.1. Stir/shakeStir/shakeTo speed up solvation. . .To speed up solvation. . .

F.F. Rate of SolvationRate of Solvation


1.1. Stir/shakeStir/shake2.2. Break apart soluteBreak apart solute

To speed up solvation. . .To speed up solvation. . .F.F. Rate of SolvationRate of Solvation


1.1. Stir/shakeStir/shake2.2. Break apart soluteBreak apart solute3.3. Heat the solventHeat the solvent

To speed up solvation. . .To speed up solvation. . .F.F. Rate of SolvationRate of Solvation

II.II. Is it soluble?Is it soluble?

II.II. Is it soluble?Is it soluble?A.A. Not all ionic compounds Not all ionic compounds

dissolve in water.dissolve in water.


1.1. Solubility TableSolubility Table

A.A. Not all ionic compounds Not all ionic compounds dissolve in water.dissolve in water.


1.1. Solubility TableSolubility Table2.2. Writing physical states Writing physical states

(in equations)(in equations)


Insoluble = (s) for solidSoluble = ______________



(in equations)(in equations)


Insoluble = (s) for solidSoluble = (aq) for aqueous



(in equations)(in equations)3.3. Solubility RulesSolubility Rules


Self Check – Ex. 1Self Check – Ex. 1

Is copper (II) chloride Is copper (II) chloride soluble?soluble?


Is zinc carbonate soluble?Is zinc carbonate soluble?


Is calcium hydroxide Is calcium hydroxide soluble?soluble?


dissolve in water.dissolve in water.B.B. In reality, ionic compounds In reality, ionic compounds

all dissolve in varying degrees.all dissolve in varying degrees.

Some compounds are very soluble while others are slightly soluble



all dissolve in varying degrees.all dissolve in varying degrees.1.1. Solubility depends on Solubility depends on

______________________

Solubility Solubility CurveCurve




temperaturetemperature2.2. Solubility depends on Solubility depends on

physical statephysical state




temperaturetemperature2.2. Solubility depends on Solubility depends on

physical statephysical state3.3. Solubility of gas depends Solubility of gas depends

on on pressurepressure

Henry’s LawHenry’s Law

The solubility (S) of a gas The solubility (S) of a gas in a liquid is directly in a liquid is directly proportional to the proportional to the pressure (P) of the gaspressure (P) of the gas

SS11

PP11

SS22

PP22

==


The solubility of OThe solubility of O22 in in water is 1.2 g/L when the water is 1.2 g/L when the pressure 2.0 atm. What is pressure 2.0 atm. What is the solubility when the the solubility when the pressure is 6.0 atm?pressure is 6.0 atm?

III.III. Heat of solutionHeat of solution

III.III. Heat of solutionHeat of solutionA.A. Many reactions warm up Many reactions warm up

when you mix substanceswhen you mix substances

Exothermic – heat given off

III.III. Heat of solutionHeat of solutionA.A. Many reactions warm up Many reactions warm up

when you mix substanceswhen you mix substancesB.B. Some reactions get colder Some reactions get colder

when you mix substanceswhen you mix substances

Endothermic – heat absorbed

IV.IV. ConcentrationConcentration

IV.IV. ConcentrationConcentrationA.A. TermsTerms


1.1. ConcentratedConcentratedA.A. TermsTerms

A solution that has a lot of per solvent

A solution that has a lot of solute per solvent


1.1. ConcentratedConcentratedA.A. TermsTerms


1.1. ConcentratedConcentrated2.2. DiluteDilute

A.A. TermsTerms

A solution that has a lot of .


1.1. ConcentratedConcentrated2.2. DiluteDilute

A.A. TermsTerms

A solution that has a lot of solvent.


1.1. ConcentratedConcentrated2.2. DiluteDilute3.3. SaturatedSaturated

A.A. TermsTerms

A solution with solute.


1.1. ConcentratedConcentrated2.2. DiluteDilute3.3. SaturatedSaturated

A.A. TermsTerms

A solution with the maximum amount of solute.

A solution with .


1.1. ConcentratedConcentrated2.2. DiluteDilute3.3. SaturatedSaturated4.4. SupersaturatedSupersaturated

A.A. TermsTerms

A solution with more solute than it can hold.


1.1. ConcentratedConcentrated2.2. DiluteDilute3.3. SaturatedSaturated4.4. SupersaturatedSupersaturated

A.A. TermsTerms

Quantifying concentrations

IV.IV. ConcentrationConcentrationA.A. TermsTermsB.B. MeasurementsMeasurements


1.1. PercentagePercentage

A.A. TermsTermsB.B. MeasurementsMeasurements




a.a. By massBy mass

mass solutemass solution

x 100

Solution = solute & solvent

Percent by mass =

Self Check – Ex. 5Self Check – Ex. 5What is the percent by What is the percent by mass when 40 g of salt is mass when 40 g of salt is added to 200 g of water.added to 200 g of water.




a.a. By massBy massb.b. By volumeBy volume

x 100Percent by volume =




a.a. By massBy massb.b. By volumeBy volume

volume solutevolume solution

x 100Percent by volume =

Self Check – Ex. 6Self Check – Ex. 6What is the percent by What is the percent by volume when 50 mL of volume when 50 mL of methanol is added to 450 methanol is added to 450 mL of water.mL of water.


1.1. PercentagePercentage2.2. MolaMolarrityity


moles solutevolume solution

x 100Molarity =

Self Check – Ex. 7Self Check – Ex. 7A solution is formed by A solution is formed by adding 7.4 g of Ca(OH)adding 7.4 g of Ca(OH)22 to to 500 mL of solution. What is 500 mL of solution. What is the molarity?the molarity?

Self Check – Ex. 8Self Check – Ex. 8How many grams of How many grams of potassium nitrate, KNOpotassium nitrate, KNO33 are required to make 250 are required to make 250 mL solution with a mL solution with a molarity of 0.40 molarity of 0.40 MM??


1.1. PercentagePercentage2.2. MolaMolarrityity3.3. MolaMolallityity


moles solutevolume solution

x 100Molality =

Self Check – Ex. 9Self Check – Ex. 9What is the molality of a What is the molality of a solution of 60 g of NaOH solution of 60 g of NaOH and 2000 g of water?and 2000 g of water?


1.1. PercentagePercentage2.2. MolaMolarrityity3.3. MolaMolallityity4.4. Mole fractionMole fraction


moles solutemoles solution

Mole fraction =

IV.IV. ConcentrationConcentrationA.A. TermsTermsB.B. MeasurementsMeasurementsC.C. Diluting solutionsDiluting solutions

M1V1 = M2V2

V.V. Solution StoichiometrySolution Stoichiometry

V.V. Solution StoichiometrySolution StoichiometryA.A. Concentrations are ratios, Concentrations are ratios,

used like conversion factorsused like conversion factors

V.V. Solution StoichiometrySolution StoichiometryA.A. Concentrations are ratios, Concentrations are ratios,

used like conversion factorsused like conversion factorsB.B. Remember the rulesRemember the rules

Stoich. RulesStoich. Rules1.1. Balance EquationBalance Equation

Stoich. RulesStoich. Rules1.1. Balance EquationBalance Equation2.2. ID units of UnknownID units of Unknown

Stoich. RulesStoich. Rules1.1. Balance EquationBalance Equation2.2. ID units of UnknownID units of Unknown3.3. Write givenWrite given

Stoich. RulesStoich. Rules1.1. Balance EquationBalance Equation2.2. ID units of UnknownID units of Unknown3.3. Write givenWrite given4.4. Insert ‘conversion factors’Insert ‘conversion factors’

Self Check – Ex. 10Self Check – Ex. 10How many grams of AgCl How many grams of AgCl are formed when a 35.5 mL are formed when a 35.5 mL sample 0.12 sample 0.12 MM AgNO AgNO33 is is added to excess NaCl added to excess NaCl solution?solution?

Self Check – Ex. 11Self Check – Ex. 11How many milliliters of How many milliliters of 0.25 0.25 MM HCl is required to HCl is required to react with 4.0 g of NaOH?react with 4.0 g of NaOH?

VI.VI. Colligative PropertiesColligative Properties

Properties affected by the number of solute particles, but not the identify of those particles

VI.VI. Colligative PropertiesColligative PropertiesA.A. Vapor Pressure: it’s loweredVapor Pressure: it’s lowered

A measure of liquid water’s ability to become a vapor

VI.VI. Colligative PropertiesColligative PropertiesA.A. Vapor Pressure: it’s loweredVapor Pressure: it’s loweredB.B. Boiling Point: it’s elevatedBoiling Point: it’s elevated

VI.VI. Colligative PropertiesColligative PropertiesA.A. Vapor Pressure: it’s loweredVapor Pressure: it’s loweredB.B. Boiling Point: it’s elevatedBoiling Point: it’s elevatedC.C. Freezing Point: it’s loweredFreezing Point: it’s lowered

VI.VI. Colligative PropertiesColligative PropertiesA.A. Vapor Pressure: it’s loweredVapor Pressure: it’s loweredB.B. Boiling Point: it’s elevatedBoiling Point: it’s elevatedC.C. Freezing Point: it’s loweredFreezing Point: it’s loweredD.D. Osmotic Pressure: it’s loweredOsmotic Pressure: it’s lowered

Osmosis is movement of water through a semi-permeable membrane

VII.VII. Heterogeneous MixturesHeterogeneous Mixtures

VII.VII. Heterogeneous MixturesHeterogeneous MixturesA.A. SuspensionsSuspensions

VII.VII. Heterogeneous MixturesHeterogeneous MixturesA.A. SuspensionsSuspensionsB.B. ColloidsColloids

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