a) What is the solute? b) What is the solvent? c) What is the state of the solution (gas, liquid, solid)? 7. What is the molality of the solution described in question #6? 8. What is the mole fraction of water from the solution described in #6?
9. Why does octane dissolve in hexane but not in water? 10. What is the concentration (M) of atmospheric O 2 dissolved in water at 30 o C? 11. The vapor pressure of pure water at 25 o C is 23.76 torr. What is the vapor pressure of a solution prepared by dissolving 28 grams of glucose (C 6 H 12 O 6 ) in 100 grams of water?
12. What is the freezing point of the solution described in question #11? 13. What is the boiling point of the solution described in question #11? 14. 100 grams of a non-ionic unknown solid is dissolved in 2000 grams of water. The resulting solution has a freezing point of -0.76 o C. What is the Molar Mass of the unknown?
Formulae you might need to know: Ideal Gas Law: P x V = n x R x T q = n x C x ∆ T q = n x ∆ H phase change Molality: c m = moles solute /kg of solvent Molarity: M = moles solute /Liter of solution Mole fraction of a substance: Χ = moles of substance / total moles Freezing Point Depression: ∆ T fp = K fp x c m x ( solute particles/solute molecule) Where K fp is the freezing point depression constant for the solvent Boiling Point Elevation: