Which of the following solution have highest boiling point. (Assume all salts completely dissociates)

Options

A. 0.1 M `Al_(2)(SO_(4))_(3)`
B. 0.1 `MBaCI_(2)`
C. 0.1 M glucose
D. 0.1 `M AlCI_(3)`

Explanation

To determine which of the given solutions has the highest boiling point, we need to consider the concept of colligative properties, specifically boiling point elevation. The boiling point elevation depends on the number of solute particles in a solution, which can be calculated using the Van't Hoff factor (i) and the molarity (C) of the solution.

### Step-by-Step Solution:

1. **Identify the Solutions and Their Dissociation:**
- 0.1 M Al₂(SO₄)₃
- 0.1 M BaCl₂
- 0.1 M Glucose
- 0.1 M AlCl₃

2. **Calculate the Van't Hoff Factor (i) for Each Solution:**
- **Al₂(SO₄)₃:**
- Dissociates into: 2 Al³⁺ + 3 SO₄²⁻
- Total ions = 2 + 3 = 5
- Van't Hoff factor (i) = 5

- **BaCl₂:**
- Dissociates into: 1 Ba²⁺ + 2 Cl⁻
- Total ions = 1 + 2 = 3
- Van't Hoff factor (i) = 3

- **Glucose:**
- Glucose does not dissociate into ions.
- Total particles = 1 (it remains as one molecule)
- Van't Hoff factor (i) = 1

- **AlCl₃:**
- Dissociates into: 1 Al³⁺ + 3 Cl⁻
- Total ions = 1 + 3 = 4
- Van't Hoff factor (i) = 4

3. **Calculate the Effective Particle Concentration (i × C) for Each Solution:**
- **Al₂(SO₄)₃:**
- Effective particles = i × C = 5 × 0.1 = 0.5

- **BaCl₂:**
- Effective particles = i × C = 3 × 0.1 = 0.3

- **Glucose:**
- Effective particles = i × C = 1 × 0.1 = 0.1

- **AlCl₃:**
- Effective particles = i × C = 4 × 0.1 = 0.4

4. **Compare the Effective Particle Concentrations:**
- Al₂(SO₄)₃: 0.5
- BaCl₂: 0.3
- Glucose: 0.1
- AlCl₃: 0.4

5. **Determine the Solution with the Highest Boiling Point:**
- The solution with the highest effective particle concentration is 0.1 M Al₂(SO₄)₃ with 0.5 particles. Therefore, it will have the highest boiling point.

### Conclusion:
The solution with the highest boiling point is **0.1 M Al₂(SO₄)₃**.

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