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PCC CH 100 - Lecture Notes

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Solutions Chapter 14Chapter Outline14.1 General Properties of SolutionsSlide 4Slide 5Properties of True SolutionsSlide 7Slide 8Slide 914.2 SolubilitySolubility describes the amount of solute that will dissolve in a specified amount of solvent.Slide 12Slide 13Slide 14Slide 1514.3 Factors Related to SolubilitySlide 17The Nature of the Solute and SolventSlide 19Slide 20Slide 21Slide 22The Effect of Temperature on SolubilityMost solutes have a limited solubility in a specific solvent at a fixed temperature.Effect of Temperature on the Solubility of a Solid in a LiquidSlide 26Slide 27Effect of Temperature on the Solubility of a Gas in WaterSlide 29The Effect of Pressure on SolubilitySlide 31Slide 32Saturated, Unsaturated and Supersaturated SolutionsSlide 34Slide 35Slide 36Slide 37Slide 3814.4 Rate of Dissolving SolidsSlide 40Slide 41Slide 42Slide 43Slide 44Slide 45Slide 4614.5 Solutions: A Reaction MediumMany solids must be put into solution to undergo appreciable chemical reactions.sodium chloride reacts with silver nitrateSlide 50Slide 51Slide 52Slide 53Slide 5414.6 Concentration of SolutionsThe concentration of a solution expresses the amount of solute dissolved in a given quantity of solvent or solution.Dilute and Concentrated SolutionsSlide 58Slide 59Mass Percent SolutionMass percent expresses the concentration of solution as the percent of solute in a given mass of solution.Slide 62Slide 63Slide 64Slide 65Mass/Volume Percent (m/v)Mass /volume percent expresses the concentration as grams of solute per 100 ml solution.Slide 68Volume PercentSolutions that are formulated from liquids are often expressed as volume percent with respect to the solute.Volumes are not necessarily additive.MolarityMolarity of a solution is the number of moles of solute per liter of solution.Molarity can be expressed in grams of solute rather than moles of solute.Slide 75Slide 76Slide 77Slide 78Slide 79Slide 80Slide 81Slide 82Dilution ProblemsSlide 84Slide 85Slide 86Slide 87Slide 88Slide 89Slide 90Slide 91Slide 9214.7 Colligative Properties of SolutionsWhen a nonvolatile solute is added to a solvent, three physical properties of the solvent will change:Colligative properties of a solution depend only on the number of solute particles in a solution and not on the nature of those particles.Slide 96Slide 97Slide 98Slide 99Slide 100MolalitySlide 102Slide 103Slide 104Slide 105Slide 106Slide 107Slide 10814.8 Osmosis and Osmotic PressureOsmosis is the diffusion of water, either from a dilute solution or from pure water, through a semipermeable membrane into a solution of higher concentration.Slide 112Slide 113Slide 114Osmtoic PressureSlide 119Slide 1201Solutions Chapter 14 Solutions Chapter 14 Hein and Arena Eugene Passer Chemistry Department Bronx Community College© John Wiley and Sons, IncVersion 2.012th Edition2Chapter Outline14.1 General Properties of Solutions14.2 Solubility14.3 Factors Related to Solubility14.4 Rate of Dissolving Solids14.5 Solutions: A Reaction Medium14.6 Concentration of Solutions14.7 Colligative Properties of Solutions14.8 Osmosis and Osmotic Pressure314.114.1General Properties of General Properties of SolutionsSolutions14.114.1General Properties of General Properties of SolutionsSolutions4•The solute is the component that is dissolved or is the least abundant component of the solution.•The solvent is the dissolving agent or the most abundant component in the solution.•A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance.56Properties of True Properties of True SolutionsSolutionsProperties of True Properties of True SolutionsSolutions7–This means that the ratio of solvent to solute can be varied.•The dissolved solute is molecular or ionic in size.•It is either colored or colorless and is usually transparent.•A mixture of two or more components–solute and solvent –is homogeneous and has a variable composition.8•The solute can generally be separated from the solvent by purely physical means such as evaporation.•The solute particles of a true solution are molecular or ionic in size.–The particle size range is 0.1 nm to 1 nm (10-8 cm to10-7cm).•The solute remains uniformly distributed throughout the solution and will not settle out with time.9solventsolutesolutionFormation of a Solution1014.214.2SolubilitySolubility14.214.2SolubilitySolubility11Solubility describes the amount of solute that will dissolve in a specified amount of solvent.12Solubilities of substances vary widely.13–very soluble–soluble–moderately soluble–slightly soluble–insoluble•Terms that describe the extent of solubility of a solute in a solvent:14•Terms that describe the solubility of liquids:–immiscible: liquids that are insoluble in each other.oil and watermethyl alcohol and water–miscible: liquids that are capable of mixing and forming homogeneous solutions.1514.2Solubility of Various Common Ions in Cold Water1614.314.3Factors Related to Factors Related to SolubilitySolubility14.314.3Factors Related to Factors Related to SolubilitySolubility17–ion size–interactions between solute and solvent–temperature•Factors that affect solubility are:18The Nature of theThe Nature of theSolute and SolventSolute and SolventThe Nature of theThe Nature of theSolute and SolventSolute and Solvent19•The general rule for predicting solubility is “like dissolves like”.20•Polar compounds tend to be more soluble in polar solvents than nonpolar solvents.SolventPolarity–NaCl (sodium chloride) is•soluble in water•slightly soluble in ethyl alcohol•insoluble in ether and benzene21Dissolution of sodium chloride in water.Polar water molecules are attracted to Na+ and Cl- ions in the salt or crystal, weakening the attraction between the ions.As the attraction between the ions weakens, the ions move apart and become surrounded by water dipoles.The hydrated ions slowly diffuse away from the crystal to become dissolved in solution.14.322•Nonpolar compounds tend to be more soluble in nonpolar solvents than in polar solvents.SolventPolarity–benzene is•insoluble in water•soluble in ether23The Effect ofThe Effect ofTemperature on SolubilityTemperature on SolubilityThe Effect ofThe Effect ofTemperature on SolubilityTemperature on Solubility24Most solutes have


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