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
Transcribed Image Text:**Problem 3:**
Compare the boiling points of the above solutions that contain 10 g of a solute. (Boiling point 1 = 101.75°C of NaCl, in 100 g of water; boiling point 2 = 100.15°C of C₁₂H₂₂O₁₁ in 100 g of water). Comment on the boiling points considering the colligative properties of solutions.
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### Explanation
This problem involves understanding the effect of colligative properties on the boiling points of solutions. Colligative properties depend on the number of solute particles in a solvent and not their identity.
**Analysis of Boiling Points:**
1. **NaCl Solution:**
- **Boiling Point 1**: 101.75°C
- NaCl is an ionic compound and dissociates into ions, increasing the number of particles in solution and, consequently, raising the boiling point significantly.
2. **C₁₂H₂₂O₁₁ Solution (Sugar):**
- **Boiling Point 2**: 100.15°C
- C₁₂H₂₂O₁₁ (sucrose) does not dissociate into ions. It acts as a nonelectrolyte, contributing fewer particles than NaCl per mole of solute, thus having a smaller effect on the boiling point.
### Colligative Properties Insight
- **Boiling Point Elevation**: A phenomenon where the boiling point of a liquid (solvent) is increased by adding a solute. This is dependent on the number of dissolved particles.
- **Effect of Ionic vs. Molecular Solutes**: Ionic solutes like NaCl dissociate in solution, producing more particles compared to non-dissociating molecular solutes like sugar.
By understanding this, students can appreciate how the type and nature of solutes affect boiling points through colligative properties.
Expert Solution
Step 1
Use boiling point elevation formula to get the answer
For NaCl=101.7°c
For sucrose
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