Which of the following solutions has the lowest boiling point? 0.15 M NaCl, 0.10 M CaCl2 0.15 M Ba(NO2)2 0.20 M C6H12O6 0.10 M Fe(NO3)3

Which member of each of the following pairs of compounds has the lower freezing point? a. 3.0 M glucose or 1.0 M NaCl b. 4.0 M NaCl or 1.0 M Na2SO4 c. 1.0 M CaCl2 or 2.0 M CaCl2 d. 2.0 M glucose or 0.50 M Na2SO4

Arrange the following solutions in order by their decreasing freezing points: 0.1 m Na3PO4, 0.1 m C2H5OH, 0.01 m CO2, 0.151 m NaCI, and 0.21 m cacI2.

Calculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.

Samples of each of the substances listed below are dissolved in 125 g of water. Which of the solutions has the highest boiling point? (a) 3.0 g sucrose, C12H22O11 (b) 1.0 g glycerol, C3H3(OH)3 (c) 1.0 g propylene glycol, C3H6(OH)2 (d) 2.0 g glucose, C6H12(OH)2

Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.

Indicate the most important types of intermolecular attractions in each of the following solutions: (a) The solution in Figure 11.2. (b) NO(I) in CO(I) (c) CI2(g) in Br2(l) (d) HCl(g) in benzene C6H6(l) (e) Methanol CH3OH(I) in H2O(I)