==What is the freezing point of the solution? (Assume that the molarity and molality are the same for this solution. Ké(H₂O) =Freezing point =-1.86 °C/m.)°C An aqueous solution containing 10.1 g of starch per liter has an osmotic pressure of 3.60 mm Hg at 25 °C.

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Answered: What is the freezing point of the…

What is the freezing point of the solution? (Assume that the molarity and molality are the same for this solution. Kfp (H₂O) = −1.86 °C/m.) Freezing point = 8 °℃

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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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.

Question

==
What is the freezing point of the solution? (Assume that the molarity and molality are the same for this solution. Ké(H₂O) =
Freezing point =
-1.86 °C/m.)
°C

An aqueous solution containing 10.1 g of starch per liter has an osmotic pressure of 3.60 mm Hg at 25 °C.

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