Question

Assuming ideal behavior, which of the following aqueous solutions would be expected to exhibit the smallest freezing-point lowering?

a. 0.1 m KCL
b. 0.05 m CH3COOOH
c. 0.05 m Al2(SO4)3
d. 0.1 m CaCl2
e. 0.25 m C6H12O6

Answer 1

The solution that would be expected to exhibit the smallest freezing-point lowering is 0.1 m glucose (C6H12O6), since it is a nonelectrolyte and does not dissociate into ions, resulting in the lowest concentration of particles.

Step-by-step explanation:

The freezing point depression is proportional to the concentration of dissolved particles. Therefore, the solution that would be expected to exhibit the smallest freezing-point lowering is the one with the lowest concentration of particles. In this case, the solution with the smallest freezing-point lowering would be 0.1 m glucose (C6H12O6), since it is a nonelectrolyte and does not dissociate into ions, resulting in the lowest concentration of particles.

Answer 2

The smallest freezing-point lowering would be expected from the 0.1 m CaCl2 solution.

Step-by-step explanation:

The freezing point depression is proportional to the concentration of dissolved particles in a solution. Based on the given information, the order of freezing points of the solutions from smallest to highest would be:

1. 0.1 m CaCl2
2. 0.05 m CH3COOOH
3. 0.1 m KCL
4. 0.05 m Al2(SO4)3
5. 0.25 m C6H12O6

The smallest freezing-point lowering would be expected from the 0.1 m CaCl2 solution.