Question

A chemist makes a solution of 1.33 mol CaCl2 and 800 kg water, and then discovers that the freezing point of the solution is significantly less than 0°C. How could the chemist change the solution to increase the freezing point?

Answer 1

A chemist makes a solution of 1.33 mol CaCl2 and 800 kg water, and then discovers that the freezing point of the solution is significantly less than 0°C. How could the chemist change the solution to increase the freezing point?

A) Let some of the water evaporate.
B) Add 200 kg of water to the solution.
C) Pour out some of the solution from its container.
D) Add 0.67 mol of CaCl2 to the solution.


Best Answer: (B) Add 200 kg of water to the solution. The reason the freezing point is less than zero is because of the colligative property and the addition of CaCl2. Evaporating water (A), would increase the concentration of CaCl2 and lower the freezing point even further. Pouring out some solution (D) won't change anything, and the solution will still freeze at the same temp. And adding more CaCl2 (E) will also decrease the freezing point even further.

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