无机化学英文ppt课件：chapter11

Chapter 11Properties of Solutions无机化学英文ppt课件：chapter11Section 11.1Solution CompositionCopyright Cengage Learning.All rights reserved2Various Types of SolutionsCopyright Cengage Learning.Section 11.1Solution CompositionCopyright Cengage Learning.All rights reserved3Solution CompositionCopyright Cengage Learning.Section 11.1Solution CompositionCopyright Cengage Learning.All rights reserved4MolarityCopyright Cengage Learning.Section 11.1Solution CompositionCopyright Cengage Learning.All rights reserved5Mass PercentCopyright Cengage Learning.Section 11.1Solution CompositionCopyright Cengage Learning.All rights reserved6Mole FractionCopyright Cengage Learning.Section 11.1Solution CompositionCopyright Cengage Learning.All rights reserved7MolalityCopyright Cengage Learning.Section 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 form the solution.Copyright Cengage Learning.All rights reserved8Formation of a Liquid SolutionSection 11.2The Energies of Solution FormationSteps in the Dissolving ProcessCopyright Cengage Learning.All rights reserved9Steps in the Dissolving ProcesSection 11.2The Energies of Solution FormationSteps in the Dissolving ProcessSteps 1 and 2 require energy,since forces 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 reserved10Steps in the Dissolving ProcesSection 11.2The Energies of Solution FormationEnthalpy(Heat)of SolutionEnthalpy change associated with the 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 reserved11Enthalpy(Heat)of SolutionEntSection 11.2The Energies of Solution FormationEnthalpy(Heat)of SolutionCopyright Cengage Learning.All rights reserved12Enthalpy(Heat)of SolutionCopSection 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!Explain why water and oil(a lSection 11.2The Energies 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 solute,nonpolar solventSmallSmallSmallSmallSolution formsPolar solute,nonpolar solventLargeSmallSmallLarge,positiveNo solution formsThe Energy Terms for Various TSection 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.Processes that require large amounts of energy tend not to occur.Overall,remember that“like dissolves like”.Copyright Cengage Learning.All rights reserved15In GeneralOne factor that favoSection 11.3Factors Affecting SolubilityStructure Effects:Polarity Pressure Effects:Henrys law Temperature Effects:Affecting aqueous solutionsCopyright Cengage Learning.All rights reserved16Structure Effects:Copyright Section 11.3Factors Affecting SolubilityStructure EffectsHydrophobic(water fearing)Non-polar substances Hydrophilic(water loving)Polar substancesCopyright Cengage Learning.All rights reserved17Structure EffectsHydrophobic(Section 11.3Factors Affecting SolubilityPressure EffectsLittle 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 reserved18Pressure EffectsLittle effect Section 11.3Factors Affecting SolubilityA Gaseous SoluteCopyright Cengage Learning.All rights reserved19A Gaseous SoluteCopyright CeSection 11.3Factors Affecting SolubilityTemperature Effects(for Aqueous Solutions)Although the solubility of most solids in water increases with temperature,the solubilities of some substances 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 reserved20Temperature Effects(for AqueoSection 11.3Factors Affecting SolubilityThe Solubilities of Several Solids as a Function of TemperatureCopyright Cengage Learning.All rights reserved21The Solubilities of Section 11.3Factors Affecting SolubilityThe Solubilities of Several Gases in WaterCopyright Cengage Learning.All rights reserved22The Solubilities of Several GaSection 11.4The Vapor Pressures of SolutionsAn Aqueous Solution and Pure Water in a Closed EnvironmentCopyright Cengage Learning.All rights reserved23An Aqueous Solution and Pure WSection 11.4The Vapor Pressures of SolutionsLiquid/Vapor EquilibriumCopyright Cengage Learning.All rights reserved24Liquid/Vapor EquilibriumCopyriSection 11.4The Vapor Pressures of SolutionsVapor Pressure Lowering:Addition of a SoluteCopyright Cengage Learning.All rights reserved25Vapor Pressure Lowering:AdditSection 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 reserved26Vapor Pressures of SolutionsNoSection 11.4The Vapor Pressures of SolutionsA Solution Obeying Raoults LawCopyright Cengage Learning.All rights reserved27A Solution Obeying Raoults LaSection 11.4The Vapor Pressures of SolutionsNonideal SolutionsLiquid-liquid solutions where both components are volatile.Modified Raoults Law:Nonideal solutions behave ideally as the mole fractions approach 0 and 1.Copyright Cengage Learning.All rights reserved28Nonideal SolutionsLiquid-liquiSection 11.4The Vapor Pressures of SolutionsVapor Pressure for a Solution of Two Volatile LiquidsCopyright Cengage Learning.All rights reserved29Vapor Pressure for a Solution Section 11.4The Vapor Pressures of SolutionsSummary of the Behavior 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)NegativePositiveEthanol-hexaneSummary of the Behavior of VarSection 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)Hexane(C6H14)and octane(C8H18)Copyright Cengage Learning.All rights reserved31CONCEPT CHECK!CONCEPT CHECK!For each of the following soluSection 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 elevation Freezing-point depressionOsmotic pressureCopyright Cengage Learning.All rights reserved32Colligative PropertiesDepend oSection 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-point elevation constantmsolute=molality of soluteCopyright Cengage Learning.All rights reserved33Boiling-Point ElevationNonvolaSection 11.5Boiling-Point Elevation and Freezing-Point DepressionBoiling Point Elevation:Liquid/Vapor EquilibriumCopyright Cengage Learning.All rights reserved34Boiling Point Elevation:LiquiSection 11.5Boiling-Point Elevation and Freezing-Point DepressionBoiling Point Elevation:Addition of a SoluteCopyright Cengage Learning.All rights reserved35Boiling Point Elevation:AdditSection 11.5Boiling-Point Elevation and Freezing-Point DepressionBoiling Point Elevation:Solution/Vapor EquilibriumCopyright Cengage Learning.All rights reserved36Boiling Point Elevation:SolutSection 11.5Boiling-Point 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 Cengage Learning.All rights reserved37Freezing-Point DepressionWhen Section 11.5Boiling-Point Elevation and Freezing-Point DepressionFreezing Point Depression:Solid/Liquid EquilibriumCopyright Cengage Learning.All rights reserved38Freezing Point Depression:SolSection 11.5Boiling-Point Elevation and Freezing-Point DepressionFreezing Point Depression:Addition of a SoluteCopyright Cengage Learning.All rights reserved39Freezing Point Depression:AddSection 11.5Boiling-Point Elevation and Freezing-Point DepressionFreezing Point Depression:Solid/Solution EquilibriumCopyright Cengage Learning.All rights reserved40Freezing Point Depression:SolSection 11.5Boiling-Point Elevation and Freezing-Point DepressionChanges in Boiling Point and Freezing Point of WaterCopyright Cengage Learning.All rights reserved41Changes in Boiling Point and FSection 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 the 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!A solution was prepared by diSection 11.5Boiling-Point Elevation and Freezing-Point DepressionYou take 20.0 g of a sucrose(C12H22O11)and NaCl mixture 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 sucrose is 0.313Copyright Cengage Learning.All rights reserved43EXERCISE!EXERCISE!You take 20.0 g of a sucrose 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 do nothing?Copyright Cengage Learning.All rights reserved44EXERCISE!EXERCISE!A plant cell has a natural coSection 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 rights reserved45Osmosis flow of solvent intoSection 11.6Osmotic PressureCopyright Cengage Learning.All rights reserved46Copyright Cengage Learning.Section 11.6Osmotic PressureOsmosisCopyright Cengage Learning.All rights reserved47OsmosisCopyright Cengage LeaSection 11.6Osmotic PressureCopyright Cengage Learning.All rights reserved48Copyright Cengage Learning.Section 11.6Osmotic PressureWhen 33.4 mg of a compound 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!When 33.4 mg of a compound isSection 11.7Colligative Properties of Electrolyte Solutionsvant Hoff Factor,iThe relationship between the moles of solute dissolved and the moles of particles in solution is usually expressed as:Copyright Cengage Learning.All rights reserved50vant Hoff Factor,iThe relatiSection 11.7Colligative Properties of Electrolyte SolutionsIon PairingAt a given instant a small percentage of the sodium and chloride ions are paired and thus count as a single particle.Copyright Cengage Learning.All rights reserved51Ion PairingAt a given instant Section 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 ion pairing does not occur).NaCli=2KNO3i=2Na3PO4i=4Copyright Cengage Learning.All rights reserved52ExamplesThe expected value forSection 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 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 reserved53Ion PairingIon pairing is mostSection 11.7Colligative Properties of Electrolyte SolutionsModified EquationsCopyright Cengage Learning.All rights reserved54Modified EquationsCopyright Section 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 reserved55A suspension of tiny particlesSection 11.8ColloidsTypes of ColloidsCopyright Cengage Learning.All rights reserved56Types of ColloidsCopyright CSection 11.8ColloidsCoagulationDestruction of a colloid.Usually accomplished either by heating or by adding an electrolyte.Copyright Cengage Learning.All rights reserved57CoagulationDestruction of a co