A 7.08 g sample of an ionic compound XCI2 is dissolved in 383 grams of asolvent. The freezing point of the solution is 1.22°C below that of puresolvent. What is the molar mass of this compound? Kf for solvent =4.36°C/m.Use 3 significant figures in this problem. Do not include the units in youranswer.

Answered: A 7.08 g sample of an ionic compound…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 7.08 g sample of an ionic compound XCI2 is dissolved in 383 grams of a
solvent. The freezing point of the solution is 1.22°C below that of pure
solvent. What is the molar mass of this compound? Kf for solvent =
4.36°C/m.
Use 3 significant figures in this problem. Do not include the units in your
answer.

Expert Solution

Step 1

The molecular weight of the solute can be calculated by using the colligative properties, depression in freezing point. The depression in the freezing point of a solution is given by:

∆T_f = i K_f m

∆T_f= 1.22^oC

i = van't Hoff factor = 3 (for ionic XCl₂)

Where m is = molality of the solution =?

K_f is = molal depression constant = 4.36^oC/m

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