CHEM 211 1st Edition Lecture 8Outline of Last Lecture I. Solutions and EntropyII. Solubility and EquilibriumIII. Factors that Affect SolubilityIV. Henry’s LawOutline of Current Lecture I. Interconverting Concentration TermsII. Colligative Properties of SolutionsIII. Vapor Pressure LoweringIV. Boiling Point ElevationV. Freezing Point DepressionCurrent LectureI. Interconverting Concentration TermsA. To convert a term based on amount (mol) to one based on mass, you need the molar mass. B. To convert a term based on mass to one based on volume, you need the solution density.C. Molality involves quantity of solvent, whereas the other concentration terms involve quantity of solution.D. To find the mass of solvent we assume the % is per 100 g of solution. Take the differencein the mass of the solute and solution for the mass of product.E. Convert grams of solute and solvent to moles before finding X.F. Use the density to find the volume of the solution.G. To find the mass of solvent we assume the % is per 100 gof solution.II. Colligative Properties of SolutionsA. Colligative properties are properties that depend on the numberof solute particles, not their chemical identity.B. The number of particles in solution can be predicted from the formula and type of the solute.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.C. An electrolyte separates into ions when it dissolves in water. D. Strong electrolytes dissociate completely while weak electrolytes dissociate very little.E. A nonelectrolyte does not dissociate to form ions. F. Each mole of dissolved compound yields 1 mole of particles in solution.III. Vapor Pressure LoweringA. The vapor pressure of a solution containing a nonvolatile nonelectrolyte is always lower than the vapor pressure of the pure solvent.B. Raoult’s law states that the vapor pressure of the solvent above the solution is proportional to the mole fraction of the solventpresent. >>C. The vapor pressure lowering is proportional tothe mole fraction of the solute present. >>IV. Boiling Point ElevationA. A solution always boils at a higher temperaturethan the pure solvent.B. This colligative property is a result of vapor pressure lowering.C. The boiling point elevation is proportional to the molality of thesolution.D. Kb is the molal boiling point elevation constant for the solvent.V. Freezing Point DepressionA. A solution always freezes at a lower temperature than the puresolvent.B. The freezing point depression is proportional to the molality ofthe solution.C. Kf is the molal freezing point depression constant for the
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