The normal freezing point of a certain liquid X is 0.5 °C, but when 4.33 g of urea are dissolved in 300. g of X, it is found that the solution freezes at -1.2 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Round your answer to 2 significant digits. -1 IC-mol kg
The normal freezing point of a certain liquid X is 0.5 °C, but when 4.33 g of urea are dissolved in 300. g of X, it is found that the solution freezes at -1.2 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Round your answer to 2 significant digits. -1 IC-mol kg
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
Chapter11: Properties Of Solutions
Section: Chapter Questions
Problem 141IP: An aqueous solution containing 0.250 mole of Q, a strong electrolyte, in 5.00 102 g water freezes...
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Calculate the molal freezing point depression constant of Kf of X.
Expert Solution
Step 1
Colligative properties depend upon the concentration of solute particles.
The molality of a solution is the number of moles of the solute upon mass of the solvent in kilogram.
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