solutions chapter 13 and 14 honors chemistry. solution definition: a homogeneous mixture of 2 or...
TRANSCRIPT
SolutionsSolutionsChapter 13 and 14Chapter 13 and 14
Honors ChemistryHonors Chemistry
SolutionSolution Definition a homogeneous mixture of 2 or Definition a homogeneous mixture of 2 or
more substances in a single physical statemore substances in a single physical state Parts solute and solvent (usually water)Parts solute and solvent (usually water)
Types of solutionsTypes of solutions
Physical states solid (alloys) liquid gasPhysical states solid (alloys) liquid gas Miscible vs ImmiscibleMiscible vs Immiscible
MiscibleMiscible - liquids that dissolve freely in one - liquids that dissolve freely in one another in any proportionanother in any proportion
ImmiscibleImmiscible - liquid solutes and solvents that are - liquid solutes and solvents that are not solublenot soluble
Dilute vs ConcentratedDilute vs Concentrated Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte Saturated Unsaturated and Saturated Unsaturated and
SupersaturatedSupersaturated
Supersaturated Solution demo
Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte
SaturatedSaturated ndash soln ndash soln containing the max containing the max amt of soluteamt of solute
UnsaturatedUnsaturated ndash soln ndash soln containing less containing less solute than a sat solute than a sat soln under the soln under the existing conditionsexisting conditions
SupersaturatedSupersaturated ndash ndash contains more contains more dissolved solute dissolved solute than a saturated than a saturated solution under the solution under the same conditionssame conditions
Solubility Curves
supersaturated solutionsupersaturated solution(stirred)(stirred)
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
SolutionSolution Definition a homogeneous mixture of 2 or Definition a homogeneous mixture of 2 or
more substances in a single physical statemore substances in a single physical state Parts solute and solvent (usually water)Parts solute and solvent (usually water)
Types of solutionsTypes of solutions
Physical states solid (alloys) liquid gasPhysical states solid (alloys) liquid gas Miscible vs ImmiscibleMiscible vs Immiscible
MiscibleMiscible - liquids that dissolve freely in one - liquids that dissolve freely in one another in any proportionanother in any proportion
ImmiscibleImmiscible - liquid solutes and solvents that are - liquid solutes and solvents that are not solublenot soluble
Dilute vs ConcentratedDilute vs Concentrated Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte Saturated Unsaturated and Saturated Unsaturated and
SupersaturatedSupersaturated
Supersaturated Solution demo
Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte
SaturatedSaturated ndash soln ndash soln containing the max containing the max amt of soluteamt of solute
UnsaturatedUnsaturated ndash soln ndash soln containing less containing less solute than a sat solute than a sat soln under the soln under the existing conditionsexisting conditions
SupersaturatedSupersaturated ndash ndash contains more contains more dissolved solute dissolved solute than a saturated than a saturated solution under the solution under the same conditionssame conditions
Solubility Curves
supersaturated solutionsupersaturated solution(stirred)(stirred)
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Types of solutionsTypes of solutions
Physical states solid (alloys) liquid gasPhysical states solid (alloys) liquid gas Miscible vs ImmiscibleMiscible vs Immiscible
MiscibleMiscible - liquids that dissolve freely in one - liquids that dissolve freely in one another in any proportionanother in any proportion
ImmiscibleImmiscible - liquid solutes and solvents that are - liquid solutes and solvents that are not solublenot soluble
Dilute vs ConcentratedDilute vs Concentrated Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte Saturated Unsaturated and Saturated Unsaturated and
SupersaturatedSupersaturated
Supersaturated Solution demo
Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte
SaturatedSaturated ndash soln ndash soln containing the max containing the max amt of soluteamt of solute
UnsaturatedUnsaturated ndash soln ndash soln containing less containing less solute than a sat solute than a sat soln under the soln under the existing conditionsexisting conditions
SupersaturatedSupersaturated ndash ndash contains more contains more dissolved solute dissolved solute than a saturated than a saturated solution under the solution under the same conditionssame conditions
Solubility Curves
supersaturated solutionsupersaturated solution(stirred)(stirred)
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Supersaturated Solution demo
Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte
SaturatedSaturated ndash soln ndash soln containing the max containing the max amt of soluteamt of solute
UnsaturatedUnsaturated ndash soln ndash soln containing less containing less solute than a sat solute than a sat soln under the soln under the existing conditionsexisting conditions
SupersaturatedSupersaturated ndash ndash contains more contains more dissolved solute dissolved solute than a saturated than a saturated solution under the solution under the same conditionssame conditions
Solubility Curves
supersaturated solutionsupersaturated solution(stirred)(stirred)
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Electrolyte vs NonelectrolyteElectrolyte vs Nonelectrolyte
SaturatedSaturated ndash soln ndash soln containing the max containing the max amt of soluteamt of solute
UnsaturatedUnsaturated ndash soln ndash soln containing less containing less solute than a sat solute than a sat soln under the soln under the existing conditionsexisting conditions
SupersaturatedSupersaturated ndash ndash contains more contains more dissolved solute dissolved solute than a saturated than a saturated solution under the solution under the same conditionssame conditions
Solubility Curves
supersaturated solutionsupersaturated solution(stirred)(stirred)
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
SaturatedSaturated ndash soln ndash soln containing the max containing the max amt of soluteamt of solute
UnsaturatedUnsaturated ndash soln ndash soln containing less containing less solute than a sat solute than a sat soln under the soln under the existing conditionsexisting conditions
SupersaturatedSupersaturated ndash ndash contains more contains more dissolved solute dissolved solute than a saturated than a saturated solution under the solution under the same conditionssame conditions
Solubility Curves
supersaturated solutionsupersaturated solution(stirred)(stirred)
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
supersaturated solutionsupersaturated solution(stirred)(stirred)
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Solubility Solubility (physical change)(physical change)
Definition mass of Definition mass of solute needed to solute needed to make a saturated make a saturated solution at a given solution at a given temperaturetemperature solution equilibrium in solution equilibrium in
a closed systema closed system dissolution harr dissolution harr
crystallizationcrystallization Unit = g solute100 g Unit = g solute100 g
HH22OO
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
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)
So
lub
ilit
y (
g1
00 g
wat
er )
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
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40oC
supersaturated
90 g
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Solubility of Solubility of solidssolids in liquids in liquids
For most solids increasing For most solids increasing temperature increases solubilitytemperature increases solubility
In general ldquolike dissolves likerdquo In general ldquolike dissolves likerdquo Depends onDepends on Type of bondingType of bonding Polarity of moleculePolarity of molecule Intermolecular forces between solute Intermolecular forces between solute
and solventand solvent
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Solubility of GasesSolubility of Gases Gases are less Gases are less
soluble at high soluble at high temperatures than temperatures than at low temperaturesat low temperatures
Increasing Increasing temperature temperature decreases solubilitydecreases solubility
Increasing pressure Increasing pressure increases solubilityincreases solubility
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
The quantity of gas that dissolves in a The quantity of gas that dissolves in a certain volume of liquid is certain volume of liquid is directly directly proportionalproportional to the pressure of the gas to the pressure of the gas (above the solution)(above the solution)
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
EffervescenceEffervescence ndash rapid escape of gas ndash rapid escape of gas dissolved in liquiddissolved in liquid
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Factors Affecting SolubilityFactors Affecting Solubility Increase surface area of solute Increase surface area of solute
(crushing)(crushing) StirshakeStirshake Increase temperatureIncrease temperature
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Dissolution ProcessDissolution Process Ionic CompoundsIonic Compounds
NaClNaCl(s)(s) Na Na+1+1(aq)(aq) + Cl + Cl-1-1
(aq)(aq)
For dissolution to occur must overcome solute attractions For dissolution to occur must overcome solute attractions and solvent attractionsand solvent attractions
DissociationDissociation Reaction Reaction the separation of IONS when an the separation of IONS when an ionic compound dissolves (ions already present)ionic compound dissolves (ions already present)
Try calcium chlorideTry 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 ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Dissolution ProcessDissolution Process Molecular CompoundsMolecular Compounds
Nonpolar molecular solids do not dissolve in Nonpolar molecular solids do not dissolve in polar solvents polar solvents
naphthalenenaphthalene Polar moleculePolar molecule
CC1212HH2222OO1111(s) (s) C C1212HH2222OO1111(aq) (aq) Molecular solvationMolecular solvation NonelectrolyteNonelectrolyte
Polar moleculePolar molecule HCl(g) HCl(g) H H+1+1(aq) + Cl(aq) + Cl-1-1(aq) or (aq) or HCl(g) + HHCl(g) + H22O O H H33OO+1+1(aq) + Cl(aq) + Cl-1-1(aq)(aq) IonizationIonization ions formed from solute molecules by ions formed from solute molecules by
action of solvent (no ions initially present)action of solvent (no ions initially present) Nonelectrolyte (HCl) Nonelectrolyte (HCl) electrolyte (ions) electrolyte (ions)
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Energy ChangesEnergy Changes Heat of solution = Heat of solution = HHsolnsoln EndothermicEndothermic
Solute particles separating in solidSolute particles separating in solid Solvent particles moving apart to allow solute to enter Solvent particles moving apart to allow solute to enter
liquidliquid Energy absorbedEnergy absorbed
ExothermicExothermic Solute particles separating in solidSolute particles separating in solid Solvent particles attracted to solvating solute particlesSolvent particles attracted to solvating solute particles Energy releasedEnergy released
HHsolnsoln = heat of solvation ndash = heat of solvation ndashcrystal lattice energycrystal lattice energy
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Solution ReactionsSolution Reactions
Single replacementSingle replacement Activity SeriesActivity Series
Double replacementDouble replacement Solubility chart (soluble vs insoluble)Solubility chart (soluble vs insoluble) Neutralization (water)Neutralization (water) Gases (COGases (CO2 2 and Hand H22S)S)
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
ConcentrationConcentration Percent concentration by mass Percent concentration by mass (mass )(mass )
(solutesolution) x 100 = Concentration(solutesolution) x 100 = Concentration MolarityMolarity (M) (M)
Moles of soluteLiters of solution = molLMoles of soluteLiters of solution = molL MolalityMolality (m) (m)
Moles of solutemass of solvent = molkgMoles of solutemass of solvent = molkg ppm and ppbppm and ppb
Used for very dilute solutionsUsed for very dilute solutions DilutionDilution ndash a process in which more solvent is ndash a process in which more solvent is
added to a solutionadded to a solution How is this solution differentHow is this solution different
Volume color molarityVolume color molarity How is it the sameHow is it the same
Same mass of solute same moles of soluteSame mass of solute same moles of solute In Dilution ONLY In Dilution ONLY MM11VV11 = M = M22VV22
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Colligative PropertiesColligative Properties
Definition physical properties of Definition physical properties of solutions that differ from properties solutions that differ from properties of its solvent of its solvent
Property depends upon the number of Property depends upon the number of solute particles in solutionsolute particles in solution
TypesTypes11 Vapor PressureVapor Pressure
22 Boiling Point ELEVATIONBoiling Point ELEVATION
33 Freezing Point DEPRESSIONFreezing Point DEPRESSION
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Vapor PressureVapor PressureA measure of the tendency of molecules to escape from a A measure of the tendency of molecules to escape from a
liquidliquid For nonvolatile liquids or solid solutesFor nonvolatile liquids or solid solutes A nonvolatile solute will typically increase the A nonvolatile solute will typically increase the
boiling point and decrease the freezing point boiling point and decrease the freezing point Adding a nonvolatile solute lowers the Adding a nonvolatile solute lowers the
concentration of water molecules at the surface concentration of water molecules at the surface of the liquid of the liquid
This lowers the tendency of the water molecules to This lowers the tendency of the water molecules to leave the solution and enter the gas phase leave the solution and enter the gas phase
Therefore the vapor pressure of the solution is LESS Therefore the vapor pressure of the solution is LESS than pure water than pure water
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
H2O H2O H2O Sugar H2O
Same Temperature
Temperature (ordmC)
Vapor P
ressu
re (kP
a)
100
40
20
60
80
100H2O solution
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Boiling Point ElevationBoiling Point Elevation
ttbb = boiling point elevation = boiling point elevation ttbb = iK = iKbbmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKbb = molal bp elevation constant = molal bp elevation constant KKbb = = 0512degC0512degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent bp of solution = bp of solvent + bp of solution = bp of solvent + ttbb
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Boiling Point Elevation and Boiling Point Elevation and Freezing Point ProblemsFreezing Point Problems
11 At what temperature will a solution begin At what temperature will a solution begin to boil if it is composed of 150 g to boil if it is composed of 150 g potassium nitrate in 350 g of waterpotassium nitrate in 350 g of water
SoluteSolute
22 At what temperature will a solution begin At what temperature will a solution begin to freeze when 180 g ammonium to freeze when 180 g ammonium phosphate is dissolved in 2000 g waterphosphate is dissolved in 2000 g water
SoluteSolute
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Freezing Point DepressionFreezing Point Depressionwhen a solution freezes the solvent solidifies as a pure when a solution freezes the solvent solidifies as a pure
substance deviates for more concentrated solutionssubstance deviates for more concentrated solutions
ttff = freezing point depression = freezing point depression ttff = iK = iKffmm
i = molality conversion factor for electrolytes i = molality conversion factor for electrolytes adjust for of ions actually present in solution adjust for of ions actually present in solution (dissociation process)(dissociation process)
KKff = molal freezing point depression constant = molal freezing point depression constant KKff = = 1858degC1858degCkg Hkg H22OO
moles of solute (ions or molecules)moles of solute (ions or molecules) m = molality = m = molality = moles solutemoles solute
kg of solventkg of solvent fp of solution = fp of solvent - fp of solution = fp of solvent - ttff
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
Osmotic PressureOsmotic Pressure The external pressure needed to stop The external pressure needed to stop
osmosisosmosis OsmosisOsmosis is the movement of solvent through a is the movement of solvent through a
semi permeable membrane from lower semi permeable membrane from lower concentration to higher concentrationconcentration to higher concentration
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-
the pressure required to allow for no the pressure required to allow for no transport of solvent across the membrane is transport of solvent across the membrane is
called the OSMOTIC pressurecalled the OSMOTIC pressure
- Solutions
- Solution
- Types of solutions
- Slide 4
- Electrolyte vs Nonelectrolyte
- Slide 6
- supersaturated solution (stirred)
- Solubility (physical change)
- Slide 9
- Solubility of solids in liquids
- Solubility of Gases
- Slide 12
- Slide 13
- Factors Affecting Solubility
- Dissolution Process
- Slide 16
- Slide 17
- Energy Changes
- Solution Reactions
- Concentration
- Colligative Properties
- Vapor Pressure A measure of the tendency of molecules to escape from a liquid
- Slide 23
- Boiling Point Elevation
- Boiling Point Elevation and Freezing Point Problems
- Freezing Point Depression when a solution freezes the solvent solidifies as a pure substance deviates for more concentrated solutions
- Osmotic Pressure
- the pressure required to allow for no transport of solvent across the membrane is called the OSMOTIC pressure
-