Which solution will have the highest boiling point ?

Options

A. `1m C_(6)H_(12)O_(6)` solution
B. 1m NaCl solution
C. 1m `BaCl_(2)` solution
D. 1m urea solution

Answer

To determine which solution will have the highest boiling point, we need to analyze the boiling point elevation, which is influenced by the van 't Hoff factor (i) and the molality (m) of the solutions. The boiling point elevation can be calculated using the formula:

\[ \Delta T_b = K_b \cdot m \cdot i \]

Where:
- \(\Delta T_b\) = elevation in boiling point
- \(K_b\) = ebullioscopic constant (a property of the solvent)
- \(m\) = molality of the solution
- \(i\) = van 't Hoff factor (number of particles the solute breaks into)

### Step-by-Step Solution:

1. **Identify the Solutions**:
- C₆H₁₂O₆ (Glucose)
- NaCl (Sodium Chloride)
- BaCl₂ (Barium Chloride)
- Urea

2. **Determine the van 't Hoff Factor (i)**:
- For **C₆H₁₂O₆ (Glucose)**: It is a non-electrolyte, so it does not dissociate. Thus, \(i = 1\).
- For **NaCl**: It dissociates into Na⁺ and Cl⁻. Therefore, \(i = 2\) (1 Na⁺ + 1 Cl⁻).
- For **BaCl₂**: It dissociates into Ba²⁺ and 2 Cl⁻. Therefore, \(i = 3\) (1 Ba²⁺ + 2 Cl⁻).
- For **Urea**: It is also a non-electrolyte, so \(i = 1\).

3. **Compare the van 't Hoff Factors**:
- C₆H₁₂O₆: \(i = 1\)
- NaCl: \(i = 2\)
- BaCl₂: \(i = 3\)
- Urea: \(i = 1\)

4. **Determine the Highest Boiling Point**:
- Since \(\Delta T_b\) is directly proportional to \(i\), the solution with the highest \(i\) will have the highest boiling point.
- From our calculations, BaCl₂ has the highest \(i = 3\).

5. **Conclusion**:
- Therefore, the solution that will have the highest boiling point is the **BaCl₂ solution**.

### Final Answer:
The solution with the highest boiling point is **BaCl₂ solution**.

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