Date post: | 02-Jan-2016 |
Category: |
Documents |
Upload: | dayna-porter |
View: | 227 times |
Download: | 5 times |
SURVEY OF CHEMISTRY I
CHEM 1151
CHAPTER 7
DR. AUGUSTINE OFORI AGYEMANAssistant professor of chemistryDepartment of natural sciences
Clayton state university
CHAPTER 7
SOLUTIONS AND COLLOIDS
- A homogeneous mixture of two or more substances
Solvent - The substance present in the greatest quantity
Solute- The other substance(s) dissolved in the solvent
SOLUTION
- Solutions can exist in any of the physical states
Solid Solution- dental fillings, metal alloys (steel), polymers
Liquid Solution- sugar in water, salt in water, wine, vinegar
Gas Solution- air (O2, Ar, etc. in N2),
- NOx, SO2, CO2 in the atmosphere
SOLUTION
- A measure of how much of a solute can be dissolved in a solventat a given temperature
- Units: grams/100 mL
ExampleSolubility of sugar in water at 20 oC is 204 g/100 mL H2O
Three factors that affect solubility- Temperature
- Pressure- Polarity
SOLUBILITY
Unsaturated Solution- More solute can still be dissolved at a given temperature
Saturated Solution- No more solute can be dissolved at a given temperature
Supersaturated Solution- Too much solute has temporarily been dissolved
(more than solute solubility)
Precipitate- Solute (solid) that falls out of solution
SOLUBILITY
- A solution contains a solvent and one or more solutes
- The ratio of solute to solvent may vary in a solution
- Solution properties change with solute to solvent ratio
- The dissolved solutes are present as individual particles (ions, atoms, or molecules)
- Solutes remain uniformly distributed throughout the solution
- Solutes are separated by physical means (evaporation, distillation)
PROPERTIES OF SOLUTIONS
- A solution in which water (H2O) is the solventNaCl solution: solvent is H2O and solute is NaCl
Hydrophilic- Substances that dissolve in water
- Water loving (NaCl)- Usually polar substances
Hydrophobic- Substances that do not dissolve well in water
- Water fearing (hydrocarbons)- Usually nonpolar substances
AQUEOUS SOLUTION
- Ions make aqueous solutions good conductors of electricity
- Solution conductivity indicates the presence of ions
AQUEOUS SOLUTION
Ionic Compounds
- Form ions in aqueous solution (dissociate into component ions)
Example- NaCl solution contains Na+ and Cl- ions
NaCl(aq) → Na+(aq) + Cl-(aq)- Each ion is surrounded by water molecules
- Good conductor of electricity
AQUEOUS SOLUTION
Solvation Process
- Ions in aqueous solution are surrounded by the H2O molecules
- The O atom in each H2O molecule has partial negative charge (δ-) - Attract positive ions
- The H atoms have partial positive charge (δ+)- Attract negative ions
- Cations and anions are prevented from recombining
- Ions disperse uniformly throughout the solution (homogeneous)
AQUEOUS SOLUTION
Molecular Compounds
- Most molecular compounds do not form ions in aqueous solution- The molecules disperse throughout the solution
- Molecules are surrounded by H2O molecules
Example- Sucrose solution contains neutral sucrose molecules
- Each molecule is surrounded by water molecules - Poor conductor of electricity
- A few molecular compounds form ions in aqueous solution- HCl dissociates into H+(aq) and Cl-(aq)
- HNO3 dissociates into H+(aq) and NO3-(aq)
AQUEOUS SOLUTION
- A solution in which another substance other than water is the solvent
ExamplesAlcohol
petroleum etherPentane
Carbon tetrachloride
NONAQUEOUS SOLUTION
The rate at which solutes dissolve can be increased by
- Grinding or crushing solute particles (size reduction)
- Heating
- Stirring or agitation
RATE OF DISSOLUTION
- The amount of solute dissolved in a given quantity of solvent or solution
Percent Concentration- Percent by mass [mass-mass percent, %(m/m)]
mass of solution = mass of solute + mass of solvent
CONCENTRATION OF SOLUTIONS
100%xsolutionofmass
soluteofmass%(m/m)
A sugar solution is made by dissolving 5.8 g of sugar in82.5 g of water. Calculate the percent by mass concentration
of sugar.
% 6.6 100%xg 82.5) (5.8
g 5.8%(m/m)
CONCENTRATION OF SOLUTIONS
volume of solution ≠ volume of solvent + volume of solute
- Due differences in bond lengths and angles
- The amount of solute dissolved in a given quantity of solvent or solution
Percent Concentration- Percent by volume [volume-volume percent, %(v/v)]
CONCENTRATION OF SOLUTIONS
100%xsolutionofvolume
soluteofvolume%(v/v)
Calculate the volume percent of solute if 345 mL of ethyl alcohol is dissolved in enough water to produce 1257 mL
of solution
CONCENTRATION OF SOLUTIONS
% 27.4 100%xmL 1257
mL 345%(v/v)
- Units are specified because they do not cancel
- The amount of solute dissolved in a given quantity of solvent or solution
Percent Concentration- Mass-volume percent [%(m/v)]
CONCENTRATION OF SOLUTIONS
100%xsolutionofvolume
soluteofmass%(m/v)
The concentration of a solution of NaCl is 0.92 %(m/v)used to dissolve drugs for intravenous use. What is the
amount, in grams, of NaCl needed to prepare 41.50 mL of the solution?
g solute = [%(m/v)] x [volume of solution (mL)]/[100 %]
= [(0.92 % g/mL) x (41.50 mL)]/(100 %)
= 0.38 g
CONCENTRATION OF SOLUTIONS
Molarity (M: molar)
- The number of moles of solute per liter of solution
Lsolutionofvolume
solutemolesMolarity
- A solution of 1.00 M (read as 1.00 molar) contains 1.00 mole of solute per liter of solution
CONCENTRATION OF SOLUTIONS
Calculate the molarity of a solution made by dissolving 2.56 g of NaCl in enough water to make 2.00 L of solution
- Calculate moles of NaCl using grams and molar mass- Convert volume of solution to liters
- Calculate molarity using moles and liters
NaClmol0.0438NaClg58.44
NaClmol1xNaClg2.56
mol/L)(orM0.0219solutionL2.00
NaClmol0.0438Molarity
CONCENTRATION OF SOLUTIONS
After dissolving 1.56 g of NaOH in a certain volume of water, the resulting solution had a concentration of 1.60 M. Calculate the
volume of the resulting NaOH solution
- Convert grams NaOH to moles using molar mass- Calculate volume (L) using moles and molarity
NaOHmol0.0380NaOHg41.00
NaOHmol1xNaOHg1.56
solutionL0.0237NaOHmol1.60
solutionLxNaOHmol0.0380solution Volume
CONCENTRATION OF SOLUTIONS
Mole Fraction
- Fraction of moles of a component of solution
CONCENTRATION OF SOLUTIONS
components all of moles total
component of molesfraction mole
Given that the total moles of an aqueous solution of NaCl andother solutes is 1.75 mol. Calculate the mole fraction of NaCl
if the solution contains 4.56 g NaCl.
NaClmol0.0780NaClg58.44
NaClmole1xNaClg4.56NaClMoles
CONCENTRATION OF SOLUTIONS
0446.0 totalmol 1.75
NaCl mol 0.0780fraction mole
DILUTION
Consider a stock solution of concentration M1 and volume V1
If water is added to dilute to a new concentration M2 and volume V2
moles before dilution = moles after dilution
M1V1 = M2V2
Calculate the volume of 3.50 M HCl needed to prepare 500.0 mL of 0.100 M HCl
(3.50 M)(V1) = (0.100 M)(500.0 mL)
V1 = 14.3 mL
CHEMICAL ANALYSIS
Calculate the concentration of NaOH solution if 24.50 mL of this base is needed to neutralize 12.00 mL of 0.225 M HCl solution
- Write balanced equation and determine mole ratio
- Calculate moles of HCl (convert mL to L)
- Determine moles of NaOH
-Calculate molarity of NaOH
NaOH + HCl → NaCl + H2O
1 mole NaOH : 1 mole HCl
Volume HCl = 12.00 mL = 0.01200 L
mole HCl = 0.225 M x 0.01200 mL = 0.00270 mol = mole NaOH
NaOHM0.110NaOHL1
NaOHmL1000x
NaOHmL24.50
NaOHmol0.00270NaOHMolarity
CHEMICAL ANALYSIS
How many grams of KOH are needed to neutralize 25.00 mL of 0.250 M H2SO4 solution
- Write balanced equation and determine mole ratio
- Calculate moles of H2SO4
- Determine moles of KOH
- Calculate grams of KOH using molar mass
CHEMICAL ANALYSIS
2KOH + H2SO4 → K2SO4 + 2H2O
2 mole KOH : 1 mole H2SO4
mole H2SO4 = 0.250 M x 0.02500 L = 0.00625 mol
Mole KOH = 2 x 0.00625 mol = 0.0125 mol
KOHg0.701KOHmol1
KOHg56.11xKOHmol0.0125KOHmass
CHEMICAL ANALYSIS
- Substances whose aqueous solutions contain ions NaCl(aq) → Na+(aq) + Cl-(aq)
- Two categories: strong and weak electrolytes
Strong Electrolytes- Solutes that completely or nearly completely
ionize when dissolved in water
Salts: NaCl, NH4Cl, KBr, NaNO3
Strong acids: HCl, HNO3, H2SO4
Strong Bases: NaOH, KOH, Ca(OH)2
ELECTROLYTES
- Substances whose aqueous solutions contain ionsNaCl(aq) → Na+(aq) + Cl-(aq)
- Two categories: strong and weak electrolytes
Weak Electrolytes- Only a small fraction of solutes ionize when
dissolved in water (exhibit a small degree of ionization)
Weak acids: acetic acid (HC2H3O2), citric acid (C6H8O7)Weak bases: ammonia (NH3) methylamine, cocaine, morphine
ELECTROLYTES
- Single arrow is used to represent ionization of strong electrolytesH2SO4(aq) → H+(aq) + HSO4
-(aq)- Ions have no tendency of recombining to form H2SO4
- Double arrow is used to represent ionization of weak electrolytesHC2H3O2(aq) ↔ H+(aq) + C2H3O2
-(aq)- This implies reaction occurs in both directions
- Chemical equilibrium is when there is a balance in both directions
ELECTROLYTES
NONELECTROLYTES
- Substances whose aqueous solutions do not contain ions
ExamplesMany molecular compounds
Sucrose (C12H22O11) ethanol (C2H5OH)
COLLIGATIVE PROPERTIES
- Physical properties of a solvent changes when a solute is added
- Four physical properties change based on the amount of solute added but not the solute’s chemical identity
- These are known as the Colligative Properties- Vapor-pressure lowering- Boiling-point elevation
- Freezing-point depression- Osmotic pressure
Osmolarity (osmol) = (M) x (i)i = number of particles produced from the dissociation
of one formula unit of solute
- The number of particles present determines the osmotic pressure
- NaCl dissociates in solution to produce 2 particles (Na+ and Cl-)
- Glucose does not dissociate - The osmotic pressure of NaCl is twice that of glucose
- Solutions with higher osmotic pressure take up more water than solutions with lower osmotic pressure
COLLIGATIVE PROPERTIES
COLLOIDAL DISPERSION
- A substance is dispersed in another substance but not dissolved(typically cloudy)
- Dispersed particles are intermediate in size between those of a
true solution and an ordinary heterogeneous mixture
- Dispersed phase is used in place of solute
- Dispersing medium is used in place of solvent
ExamplesBlood, milk, smoke, fog, cheese, shaving cream
- The dispersed phase do not settle out under the influence of gravity and cannot be filtered out with filter paper
- Difficult to distinguish with the naked eye but scatters a beam of light
(Tyndall effect)
COLLOIDAL DISPERSION
- The passage of ions and small molecules through semipermeable membranes
- The semipermeable membrane is known as the dialyzing membrane
- The membrane holds back colloid particles and large molecules but allows solvent, hydrated ions, and small
molecules to pass through
- This technique is used to clean blood of people with kidneymalfunction
DIALYSIS