Chemistry Practice Problems Freezing Point Depression Practice Problems Solution: The freezing-point depression of a 0.091-m solutio...

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Solution: The freezing-point depression of a 0.091-m solution of CsCl is 0.320˚C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440˚C. In which solution does ion association appear to be greater? Explain.

Problem

The freezing-point depression of a 0.091-m solution of CsCl is 0.320˚C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440˚C. In which solution does ion association appear to be greater? Explain.

Solution

The problem asks us to find which solution has a greater ion association using freezing point depression data. We can determine which has a greater ion association indirectly from the  Van’t Hoff factor The Van’t Hoff factor is the number of ions created once the compound dissociates. A higher Van't Hoff factor means greater dissociation and lesser association. Inversely, a lower Van't Hoff factor means greater ion association.


The freezing point depression equation is:


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