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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![**Question 3:**
If 122.3 grams of strontium chloride is mixed with 925.0 grams of water, what will the freezing and boiling point of the resulting solution be?
---
**Description:**
This problem involves finding the freezing and boiling points of a solution when a given amount of strontium chloride (SrCl₂) is dissolved in a given mass of water (H₂O). This is a typical colligative properties problem, which depends on the number of particles in the solution rather than the type of particles.
**Key Concepts:**
1. **Freezing Point Depression:** When a solute is dissolved in a solvent, the freezing point of the solvent decreases. This can be calculated using the formula:
\[
\Delta T_f = i \cdot K_f \cdot m
\]
Where:
- \(\Delta T_f\) is the freezing point depression.
- \(i\) is the van't Hoff factor (number of particles the solute splits into).
- \(K_f\) is the freezing point depression constant of the solvent.
- \(m\) is the molality of the solution.
2. **Boiling Point Elevation:** When a solute is dissolved in a solvent, the boiling point of the solvent increases. This can be calculated using the formula:
\[
\Delta T_b = i \cdot K_b \cdot m
\]
Where:
- \(\Delta T_b\) is the boiling point elevation.
- \(i\) is the van't Hoff factor.
- \(K_b\) is the boiling point elevation constant of the solvent.
- \(m\) is the molality of the solution.
**Solution Steps:**
1. **Calculate molality (\( m \)) of the solution.**
2. **Determine the van't Hoff factor (\( i \)) for strontium chloride (SrCl₂).**
3. **Use the provided constants \( K_f \) and \( K_b \) for water.**
4. **Apply the formulas for freezing point depression and boiling point elevation to find the new freezing and boiling points.**
---
This example demonstrates how to use the properties of solutions to determine changes in physical properties like boiling and freezing points when a solute is added to a solvent.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2609b9a-bccc-4ea0-ab3c-7cfd8cf7907c%2F8f819eea-97a0-4124-93b4-e90aa29a13ab%2Fr58486n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 3:**
If 122.3 grams of strontium chloride is mixed with 925.0 grams of water, what will the freezing and boiling point of the resulting solution be?
---
**Description:**
This problem involves finding the freezing and boiling points of a solution when a given amount of strontium chloride (SrCl₂) is dissolved in a given mass of water (H₂O). This is a typical colligative properties problem, which depends on the number of particles in the solution rather than the type of particles.
**Key Concepts:**
1. **Freezing Point Depression:** When a solute is dissolved in a solvent, the freezing point of the solvent decreases. This can be calculated using the formula:
\[
\Delta T_f = i \cdot K_f \cdot m
\]
Where:
- \(\Delta T_f\) is the freezing point depression.
- \(i\) is the van't Hoff factor (number of particles the solute splits into).
- \(K_f\) is the freezing point depression constant of the solvent.
- \(m\) is the molality of the solution.
2. **Boiling Point Elevation:** When a solute is dissolved in a solvent, the boiling point of the solvent increases. This can be calculated using the formula:
\[
\Delta T_b = i \cdot K_b \cdot m
\]
Where:
- \(\Delta T_b\) is the boiling point elevation.
- \(i\) is the van't Hoff factor.
- \(K_b\) is the boiling point elevation constant of the solvent.
- \(m\) is the molality of the solution.
**Solution Steps:**
1. **Calculate molality (\( m \)) of the solution.**
2. **Determine the van't Hoff factor (\( i \)) for strontium chloride (SrCl₂).**
3. **Use the provided constants \( K_f \) and \( K_b \) for water.**
4. **Apply the formulas for freezing point depression and boiling point elevation to find the new freezing and boiling points.**
---
This example demonstrates how to use the properties of solutions to determine changes in physical properties like boiling and freezing points when a solute is added to a solvent.
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