**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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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

**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/m

The 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.

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