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.

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FREE Expert 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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Problem Details

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.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Freezing Point Depression concept. If you need more Freezing Point Depression practice, you can also practice Freezing Point Depression practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Yang's class at UT.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.