The freezing point of ethanol (C2H§OH) is -114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C) of a solution prepared by dissolving 59.1 g of glycerin (C3HgO3, a nonelectrolyte) in 400.0 g of ethanol? The molar mass of ethanol is 46.068 g/mol. Enter your answer with 1 decimal place and no unit.
The freezing point of ethanol (C2H§OH) is -114.6 °C. The molal freezing point depression constant for ethanol is 2.00 °C/m. What is the freezing point (°C) of a solution prepared by dissolving 59.1 g of glycerin (C3HgO3, a nonelectrolyte) in 400.0 g of ethanol? The molar mass of ethanol is 46.068 g/mol. Enter your answer with 1 decimal place and no unit.
Chemistry
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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
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![### Freezing Point Depression in Solutions
**Problem Statement:**
The freezing point of ethanol (C₂H₅OH) is -114.6 °C. The molal freezing point depression constant (Kf) for ethanol is 2.00 °C/m. Calculate the freezing point (°C) of a solution prepared by dissolving 59.1 g of glycerin (C₃H₈O₃, a nonelectrolyte) in 400.0 g of ethanol.
The molar mass of ethanol is 46.068 g/mol.
**Solution Requirements:**
To solve this problem, follow these steps:
1. **Calculate the molality of the solution:**
- Molality (m) is defined as the moles of solute (glycerin) per kilogram of solvent (ethanol).
- Number of moles of glycerin can be found using its molecular weight.
2. **Determine the freezing point depression:**
- Use the formula \(\Delta T_f = K_f \times m\), where \(\Delta T_f\) is the freezing point depression.
3. **Calculate the new freezing point:**
- Subtract the freezing point depression from the pure solvent's freezing point.
**Enter your answer with 1 decimal place and no unit.**
**Answer:**
```
[ ]
```](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc3a94610-8435-45dc-8284-8838c9e43692%2Fdf130b20-4c11-4843-a3ff-6a839d4ce0c4%2F7qg4iq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Freezing Point Depression in Solutions
**Problem Statement:**
The freezing point of ethanol (C₂H₅OH) is -114.6 °C. The molal freezing point depression constant (Kf) for ethanol is 2.00 °C/m. Calculate the freezing point (°C) of a solution prepared by dissolving 59.1 g of glycerin (C₃H₈O₃, a nonelectrolyte) in 400.0 g of ethanol.
The molar mass of ethanol is 46.068 g/mol.
**Solution Requirements:**
To solve this problem, follow these steps:
1. **Calculate the molality of the solution:**
- Molality (m) is defined as the moles of solute (glycerin) per kilogram of solvent (ethanol).
- Number of moles of glycerin can be found using its molecular weight.
2. **Determine the freezing point depression:**
- Use the formula \(\Delta T_f = K_f \times m\), where \(\Delta T_f\) is the freezing point depression.
3. **Calculate the new freezing point:**
- Subtract the freezing point depression from the pure solvent's freezing point.
**Enter your answer with 1 decimal place and no unit.**
**Answer:**
```
[ ]
```
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