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: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.98QE

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Concept explainers

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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