Question

The experimentally measured freezing point of a 1.30 m aqueous solution of CaCl2 is -5.80°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C. a) What is the value of the van't Hoff factor for this solution? b) What is the predicted freezing point if there were no ion clustering in the solution?

Name: the experimentally measured freezing point of a 130 m aqueous solution of cacl2 is 580c the freezing point depression constant for water is kf 186cm assume the freezing point of pure water i 47308
Uploaded: 2023-02-04T22:35:31-08:00
Duration: 1 min 39 s
Channel: David Collins
Description: the experimentally measured freezing point of a 130 m aqueous solution of cacl2 is 580c the freezing point depression constant for water is kf 186cm assume the freezing point of pure water i 47308

          The experimentally measured freezing point of a 1.30 m aqueous solution of CaCl2 is -5.80°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C.
a) What is the value of the van't Hoff factor for this solution?
b) What is the predicted freezing point if there were no ion clustering in the solution?

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Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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The experimentally measured freezing point of a 1.30 m aqueous solution of CaCl2 is -5.80°C. The freezing point depression constant for water is Kf = 1.86°C/m. Assume the freezing point of pure water is 0.00°C. a) What is the value of the van't Hoff factor for this solution? b) What is the predicted freezing point if there were no ion clustering in the solution?