All of the following are added to five different containers of water, each with the same mass of water. Which resulting solution would yield the lowest freezing point? O 2.0 mol of FeCl3 O 3.0 mol of NaNO3 O 2.0 mol of RbSO4 O 1.0 mol of KBr O 0.5 mol of C5H10O5

Instead of using NaCl to melt the ice on your sidewalk you decide to use CaCl2. If you add 35.0 g of CaCl2 to 150. g of water, what is the freezing point of the solution? (Assume i = 2.7 for CaCl2.)

For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C

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.

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

A 12.0-g sample of a nonelectrolyte is dissolved in 80.0 g of water. The solution freezes at -1.94 C. Calculate the molar mass of the substance.

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

a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. Lattice Energy Hsoln CaCl2(s) 2247kj/mol 46kj/mol Cal2(s) 2059kj/mol 104kj/mol b. Based on your answers to part a, which ion, Cl or I, is more strongly attracted to water?

A sample of aluminum sulfate 18-hydrate, Al2(SO4)3. 18H2O, containing 125.0 mg is dissolved in 1.000 L of solution. Calculate the following for the solution: a The molarity of Al2(SO4)3. b The molarity of SO42. c The molality of Al2(SO4)3, assuming that the density of the solution is 1.00 g/mL.

Will red blood cells swell, remain the same size, or shrink when placed in each of the solutions in Problem 8-101? Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? a. 0.92%(m/v) glucose solution b. 0.92%(m/v) NaCl solution c. 2.3%(m/v) glucose solution d. 5.0%(m/v) NaCl solution