Question

The experimentally measured freezing point of a 1.45 m aqueous solution of ZnCl2 is -7.28°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. What is the value of the van't Hoff factor for this solution? What is the predicted freezing point if there were no ion clustering in the solution?

Name: the experimentally measured freezing point of a 145 m aqueous solution of zncl2 is 728c the freezing point depression constant for water is kf 186cm assume the freezing point of pure water i 62715
Uploaded: 2023-02-08T16:50:53-08:00
Duration: 1 min 41 s
Channel: Sri K
Description: the experimentally measured freezing point of a 145 m aqueous solution of zncl2 is 728c the freezing point depression constant for water is kf 186cm assume the freezing point of pure water i 62715

          The experimentally measured freezing point of a 1.45 m aqueous solution of ZnCl2 is -7.28°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. What is the value of the van't Hoff factor for this solution? 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 1.45 m aqueous solution of ZnCl2 is -7.28°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. What is the value of the van't Hoff factor for this solution? What is the predicted freezing point if there were no ion clustering in the solution?