无机化学英文ppt课件：chapter11.ppt

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1、Chapter 11Properties of SolutionsSection 11.1Solution CompositionCopyright Cengage Learning.All rights reserved2Various Types of SolutionsSection 11.1Solution CompositionCopyright Cengage Learning.All rights reserved3Solution CompositionSection 11.1Solution CompositionCopyright Cengage Learning.All

2、rights reserved4MolaritySection 11.1Solution CompositionCopyright Cengage Learning.All rights reserved5Mass PercentSection 11.1Solution CompositionCopyright Cengage Learning.All rights reserved6Mole FractionSection 11.1Solution CompositionCopyright Cengage Learning.All rights reserved7MolalitySectio

3、n 11.2The Energies of Solution FormationFormation of a Liquid Solution1.Separating the solute into its individual components(expanding the solute).2.Overcoming intermolecular forces in the solvent to make room for the solute(expanding the solvent).3.Allowing the solute and solvent to interact to for

4、m the solution.Copyright Cengage Learning.All rights reserved8Section 11.2The Energies of Solution FormationSteps in the Dissolving ProcessCopyright Cengage Learning.All rights reserved9Section 11.2The Energies of Solution FormationSteps in the Dissolving ProcessSteps 1 and 2 require energy,since fo

5、rces must be overcome to expand the solute and solvent.Step 3 usually releases energy.Steps 1 and 2 are endothermic,and step 3 is often exothermic.Copyright Cengage Learning.All rights reserved10Section 11.2The Energies of Solution FormationEnthalpy(Heat)of SolutionEnthalpy change associated with th

6、e formation of the solution is the sum of the H values for the steps:Hsoln=H1+H2+H3Hsoln may have a positive sign(energy absorbed)or a negative sign(energy released).Copyright Cengage Learning.All rights reserved11Section 11.2The Energies of Solution FormationEnthalpy(Heat)of SolutionCopyright Cenga

7、ge Learning.All rights reserved12Section 11.2The Energies of Solution FormationExplain why water and oil(a long chain hydrocarbon)do not mix.In your explanation,be sure to address how H plays a role.Copyright Cengage Learning.All rights reserved13CONCEPT CHECK!CONCEPT CHECK!Section 11.2The Energies

8、of Solution FormationThe Energy Terms for Various Types of Solutes and SolventsCopyright Cengage Learning.All rights reserved14H1H2H3HsolnOutcomePolar solute,polar solventLargeLargeLarge,negativeSmallSolution formsNonpolar solute,polar solventSmallLargeSmallLarge,positiveNo solution formsNonpolar so

9、lute,nonpolar solventSmallSmallSmallSmallSolution formsPolar solute,nonpolar solventLargeSmallSmallLarge,positiveNo solution formsSection 11.2The Energies of Solution FormationIn GeneralOne factor that favors a process is an increase in probability of the state when the solute and solvent are mixed.

10、Processes that require large amounts of energy tend not to occur.Overall,remember that“like dissolves like”.Copyright Cengage Learning.All rights reserved15Section 11.3Factors Affecting SolubilityStructure Effects:Polarity Pressure Effects:Henrys law Temperature Effects:Affecting aqueous solutionsCo

11、pyright Cengage Learning.All rights reserved16Section 11.3Factors Affecting SolubilityStructure EffectsHydrophobic(water fearing)Non-polar substances Hydrophilic(water loving)Polar substancesCopyright Cengage Learning.All rights reserved17Section 11.3Factors Affecting SolubilityPressure EffectsLittl

12、e effect on solubility of solids or liquidsHenrys law:C=kPC=concentration of dissolved gask=constantP=partial pressure of gas solute above the solutionAmount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution.Copyright Cengage Learning.All rights re

13、served18Section 11.3Factors Affecting SolubilityA Gaseous SoluteCopyright Cengage Learning.All rights reserved19Section 11.3Factors Affecting SolubilityTemperature Effects(for Aqueous Solutions)Although the solubility of most solids in water increases with temperature,the solubilities of some substa

14、nces decrease with increasing temperature.Predicting temperature dependence of solubility is very difficult.Solubility of a gas in solvent typically decreases with increasing temperature.Copyright Cengage Learning.All rights reserved20Section 11.3Factors Affecting SolubilityThe Solubilities of Sever

15、al Solids as a Function of TemperatureCopyright Cengage Learning.All rights reserved21Section 11.3Factors Affecting SolubilityThe Solubilities of Several Gases in WaterCopyright Cengage Learning.All rights reserved22Section 11.4The Vapor Pressures of SolutionsAn Aqueous Solution and Pure Water in a

16、Closed EnvironmentCopyright Cengage Learning.All rights reserved23Section 11.4The Vapor Pressures of SolutionsLiquid/Vapor EquilibriumCopyright Cengage Learning.All rights reserved24Section 11.4The Vapor Pressures of SolutionsVapor Pressure Lowering:Addition of a SoluteCopyright Cengage Learning.All

17、 rights reserved25Section 11.4The Vapor Pressures of SolutionsVapor Pressures of SolutionsNonvolatile solute lowers the vapor pressure of a solvent.Raoults Law:Psoln=observed vapor pressure of solution solv=mole fraction of solvent=vapor pressure of pure solventCopyright Cengage Learning.All rights

18、reserved26Section 11.4The Vapor Pressures of SolutionsA Solution Obeying Raoults LawCopyright Cengage Learning.All rights reserved27Section 11.4The Vapor Pressures of SolutionsNonideal SolutionsLiquid-liquid solutions where both components are volatile.Modified Raoults Law:Nonideal solutions behave

19、ideally as the mole fractions approach 0 and 1.Copyright Cengage Learning.All rights reserved28Section 11.4The Vapor Pressures of SolutionsVapor Pressure for a Solution of Two Volatile LiquidsCopyright Cengage Learning.All rights reserved29Section 11.4The Vapor Pressures of SolutionsSummary of the B

20、ehavior of Various Types of SolutionsCopyright Cengage Learning.All rights reserved30Interactive Forces Between Solute(A)and Solvent(B)ParticlesHsolnT for Solution FormationDeviation from Raoults LawExampleA A,B B A BZeroZeroNone(ideal solution)Benzene-tolueneA A,B B A BPositive(endothermic)Negative

21、PositiveEthanol-hexaneSection 11.4The Vapor Pressures of SolutionsFor each of the following solutions,would you expect it to be relatively ideal(with respect to Raoults Law),show a positive deviation,or show a negative deviation?a)Hexane(C6H14)and chloroform(CHCl3)b)Ethyl alcohol(C2H5OH)and waterc)H

22、exane(C6H14)and octane(C8H18)Copyright Cengage Learning.All rights reserved31CONCEPT CHECK!CONCEPT CHECK!Section 11.5Boiling-Point Elevation and Freezing-Point DepressionColligative PropertiesDepend only on the number,not on the identity,of the solute particles in an ideal solution:Boiling-point ele

23、vation Freezing-point depressionOsmotic pressureCopyright Cengage Learning.All rights reserved32Section 11.5Boiling-Point Elevation and Freezing-Point DepressionBoiling-Point ElevationNonvolatile solute elevates the boiling point of the solvent.T=KbmsoluteT=boiling-point elevationKb=molal boiling-po

24、int elevation constantmsolute=molality of soluteCopyright Cengage Learning.All rights reserved33Section 11.5Boiling-Point Elevation and Freezing-Point DepressionBoiling Point Elevation:Liquid/Vapor EquilibriumCopyright Cengage Learning.All rights reserved34Section 11.5Boiling-Point Elevation and Fre

25、ezing-Point DepressionBoiling Point Elevation:Addition of a SoluteCopyright Cengage Learning.All rights reserved35Section 11.5Boiling-Point Elevation and Freezing-Point DepressionBoiling Point Elevation:Solution/Vapor EquilibriumCopyright Cengage Learning.All rights reserved36Section 11.5Boiling-Poi

26、nt Elevation and Freezing-Point DepressionFreezing-Point DepressionWhen a solute is dissolved in a solvent,the freezing point of the solution is lower than that of the pure solvent.T=KfmsoluteT=freezing-point depressionKf=molal freezing-point depression constantmsolute=molality of soluteCopyright Ce

27、ngage Learning.All rights reserved37Section 11.5Boiling-Point Elevation and Freezing-Point DepressionFreezing Point Depression:Solid/Liquid EquilibriumCopyright Cengage Learning.All rights reserved38Section 11.5Boiling-Point Elevation and Freezing-Point DepressionFreezing Point Depression:Addition o

28、f a SoluteCopyright Cengage Learning.All rights reserved39Section 11.5Boiling-Point Elevation and Freezing-Point DepressionFreezing Point Depression:Solid/Solution EquilibriumCopyright Cengage Learning.All rights reserved40Section 11.5Boiling-Point Elevation and Freezing-Point DepressionChanges in B

29、oiling Point and Freezing Point of WaterCopyright Cengage Learning.All rights reserved41Section 11.5Boiling-Point Elevation and Freezing-Point DepressionA solution was prepared by dissolving 25.00 g of glucose in 200.0 g water.The molar mass of glucose is 180.16 g/mol.What is the boiling point of th

30、e resulting solution(in C)?Glucose is a molecular solid that is present as individual molecules in solution.100.35 CCopyright Cengage Learning.All rights reserved42EXERCISE!EXERCISE!Section 11.5Boiling-Point Elevation and Freezing-Point DepressionYou take 20.0 g of a sucrose(C12H22O11)and NaCl mixtu

31、re and dissolve it in 1.0 L of water.The freezing point of this solution is found to be-0.426C.Assuming ideal behavior,calculate the mass percent composition of the original mixture,and the mole fraction of sucrose in the original mixture.72.8%sucrose and 27.2%sodium chloride;mole fraction of the su

32、crose is 0.313Copyright Cengage Learning.All rights reserved43EXERCISE!EXERCISE!Section 11.5Boiling-Point Elevation and Freezing-Point DepressionA plant cell has a natural concentration of 0.25 m.You immerse it in an aqueous solution with a freezing point of 0.246C.Will the cell explode,shrivel,or d

33、o nothing?Copyright Cengage Learning.All rights reserved44EXERCISE!EXERCISE!Section 11.6Osmotic PressureOsmosis flow of solvent into the solution through a semipermeable membrane.=MRT=osmotic pressure(atm)M=molarity of the solutionR=gas law constantT=temperature(Kelvin)Copyright Cengage Learning.All

34、 rights reserved45Section 11.6Osmotic PressureCopyright Cengage Learning.All rights reserved46Section 11.6Osmotic PressureOsmosisCopyright Cengage Learning.All rights reserved47Section 11.6Osmotic PressureCopyright Cengage Learning.All rights reserved48Section 11.6Osmotic PressureWhen 33.4 mg of a c

35、ompound is dissolved in 10.0 mL of water at 25C,the solution has an osmotic pressure of 558 torr.Calculate the molar mass of this compound.111 g/molCopyright Cengage Learning.All rights reserved49EXERCISE!EXERCISE!Section 11.7Colligative Properties of Electrolyte Solutionsvant Hoff Factor,iThe relat

36、ionship between the moles of solute dissolved and the moles of particles in solution is usually expressed as:Copyright Cengage Learning.All rights reserved50Section 11.7Colligative Properties of Electrolyte SolutionsIon PairingAt a given instant a small percentage of the sodium and chloride ions are

37、 paired and thus count as a single particle.Copyright Cengage Learning.All rights reserved51Section 11.7Colligative Properties of Electrolyte SolutionsExamplesThe expected value for i can be determined for a salt by noting the number of ions per formula unit(assuming complete dissociation and that i

38、on pairing does not occur).NaCli=2KNO3i=2Na3PO4i=4Copyright Cengage Learning.All rights reserved52Section 11.7Colligative Properties of Electrolyte SolutionsIon PairingIon pairing is most important in concentrated solutions.As the solution becomes more dilute,the ions are farther apart and less ion

39、pairing occurs.Ion pairing occurs to some extent in all electrolyte solutions.Ion pairing is most important for highly charged ions.Copyright Cengage Learning.All rights reserved53Section 11.7Colligative Properties of Electrolyte SolutionsModified EquationsCopyright Cengage Learning.All rights reser

40、ved54Section 11.8ColloidsA suspension of tiny particles in some medium.Tyndall effect scattering of light by particles.Suspended particles are single large molecules or aggregates of molecules or ions ranging in size from 1 to 1000 nm.Copyright Cengage Learning.All rights reserved55Section 11.8ColloidsTypes of ColloidsCopyright Cengage Learning.All rights reserved56Section 11.8ColloidsCoagulationDestruction of a colloid.Usually accomplished either by heating or by adding an electrolyte.Copyright Cengage Learning.All rights reserved57