Question

The experimentally measured freezing point of a 1.40 m aqueous solution of ZnCl2 is -7.03°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. Part 1: What is the value of the van't Hoff factor for this solution? Part 2: What is the predicted freezing point if there were no ion clustering in the solution?

Name: the experimentally measured freezing point of a 140 m aqueous solution of zncl2 is 703c the freezing point depression constant for water is kf 186cm assume the freezing point of pure water i 36751
Uploaded: 2022-02-05T06:22:20-08:00
Duration: 3 min 5 s
Channel: Jital V
Description: the experimentally measured freezing point of a 140 m aqueous solution of zncl2 is 703c the freezing point depression constant for water is kf 186cm assume the freezing point of pure water i 36751

          The experimentally measured freezing point of a 1.40 m aqueous solution of ZnCl2 is -7.03°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.

Part 1: What is the value of the van't Hoff factor for this solution?

Part 2: What is the predicted freezing point if there were no ion clustering in the solution?

Added by Angela L.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Jital V

02/05/2022

Step 1

03°C KF = 1.86°C/m M = 1.40 mol/L Calculate i: i = ΔTF / (KF * M) i = -7.03 / (1.86 * 1.40) i ≈ 2.70 Show more…

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The experimentally measured freezing point of a 1.40 m aqueous solution of ZnCl2 is -7.03°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. Part 1: What is the value of the van't Hoff factor for this solution? Part 2: What is the predicted freezing point if there were no ion clustering in the solution?