The normal freezing point of a certain liquid X is -2.7 °C, but when 12.2 g of urea ((NH,),CO) are dissolved in 500. g of 2 X, it is found that the solution freezes at -5.0 °C instead. Use this information to calculate the molal freezing point depression constant K, of X.

The normal freezing point of a certain liquid X is -2.7 °C, but when 12.2 g of urea ((NH,),CO) are dissolved in 500. g of 2 X, it is found that the solution freezes at -5.0 °C instead. Use this information to calculate the molal freezing point depression constant K, of X.

Chemistry

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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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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

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The normal freezing point of a certain liquid X is -2.7 °C, but when 12.2 g of urea
(NH,) CÓ) are dissolved in 500. g of
X, it is found that the solution freezes at -5.0 °C instead. Use this information to calculate the molal freezing point
depression constant K, of X.
Round your answer to 2 significant digits.
olo
Ar
- 1
II °C• mol
· kg
x10

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