**Problem Statement**What is the freezing point of a solution prepared by dissolving 63.49 g of glycerin (C₃H₈O₃) in 100 g of ethanol? The freezing point of ethanol (C₂H₅OH) is -114.1 °C. The freezing point depression constant for ethanol is 1.99 °C/m.---**Explanation**In this problem, we're asked to calculate the freezing point of a solution using the concept of freezing point depression. This is a colligative property that depends on the number of solute particles in a solution. The data provided includes:- Mass of glycerin: 63.49 g- Mass of ethanol: 100 g- Freezing point of pure ethanol: -114.1 °C- Freezing point depression constant for ethanol: 1.99 °C/mThe formula for freezing point depression is:\[ \Delta T_f = i \cdot K_f \cdot m \]Where:- $ \Delta T_f $ is the decrease in freezing point.- $ i $ is the van't Hoff factor (for glycerin, it is 1 because it does not ionize in solution).- $ K_f $ is the freezing point depression constant.- $ m $ is the molality of the solution.

The freezing point of pure ethanol is -114.1˚C. The amount of glycerin added to 100 g of ethanol is…

What is the freezing point of a solution prepared by dissolving 63.49 g of glycerin (C3H3O3) in 100.g ethanol? The freezing point of ethanol (C2H5OH) is-114.1 °C. The freezing point depression constant for ethanol is 1.99 °C/m.

What is the freezing point of a solution prepared by dissolving 63.49 g of glycerin (C3H3O3) in 100.g ethanol? The freezing point of ethanol (C2H5OH) is-114.1 °C. The freezing point depression constant for ethanol is 1.99 °C/m.

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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