1. A solution is prepared by mixing 1.00 g ethanol( C2H5OH) with 100.0 g water to give a final volume of 101 ml. Calculate the molarity, mass percent, mole fraction, and molality of ethanol in this solution.
  1. The electrolyte in automobile lead storage batteries is a 3.75 M sulfuric acid solution that has a density of 1.230 g/ml. Calculate the mass percent, and molality of the sulfuric acid.
  1. Decide whether liquid hexane or liquid methanol is the more appropriate solvent for the substance grease (C20H42) and potassium iodide.
  1. Calculate the enthalpy of solution for NaOH. DHf° (s) = -425.6 kJ/mol and DHf° (aq) 1m = -470.1 kJ/mol
  1. A certain soft drink is bottled so that a bottle at 25 °C contains CO2 gas at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of CO2 in the atmosphere is 4.0 x 10-4 atm, calculate the equilibrium concentrations of CO2 in the bottle both before and after the bottle is opened. The Henry’s law constant for CO2 in aqueous solution is 3.1 x 10-2 mol/atm•L at 25°C.

6. Glycerin, C3H8O3, is a nonvolatile nonelectrolyte with a density of 1.26 g/ml at 25 °C. Calculate the vapor pressure at 25C of a solution made by adding 50.0 ml of glycerin to 500.0 ml of water. The vapor pressure of pure water at 25 °C is 23.8 torr.

  1. At 40 C, the vapor pressure of pure heptane is 92.0 torr and the vapor pressure of pure octane is 31.0 torr. Consider a solution that contains 1.00 mol of heptane and 4.00 mol of octane. Calculate the total vapor pressure of each component and the total vapor pressure above the solution. Is this considered an ideal solution? Think of the type of substances in the solution.
  1. Antifreeze consists of ethylene glycol, C2H6O2, a nonvolatile nonelectrolyte. Calculate the boiling point of a 25.0 mass percent solution of ethylene glycol in water. Kb = .52 °C/m
  1. When 15.0 g of ethyl alcohol, C2H5OH is dissolved in 750. g of formic acid, the freezing point of the solution is 7.20 °C. The freezing point of pure formic acid is 8.40 °C. Evaluate the Kf for formic acid.
  1. A 1.20 g sample of an unknown compound is dissolved in 50.0 g of benzene. The solution freezes at 4.92 °C. Calculate the molecular mass of the compound. The freezing point of pure benzene is 5.48 °C and the Kf is 5.12 °C/m.
  1. Estimate the freezing point of .20m solution of Cr(NO3) 3 in water. Kf = 1.86 °C/m
  1. List the following solutions in order of their freezing points (from lowest to highest)

.050 m CaCl2, .15 m NaCl, .10 m HCl, .050 m HC2H3O2, .10 m C12H22O1