Which of the following will have highest boiling point at 1 atm pressure ?

Options

A. 0.1 M NaCl
B. 0.1 M Sucrose
C. `0.1 M BaCl_(2)`
D. 0.1 M Glucose

Explanation

To determine which of the given solutions will have the highest boiling point at 1 atm pressure, we need to consider the concept of boiling point elevation, which is influenced by the van 't Hoff factor (i), the ebullioscopic constant (Kb), and the molality (M) of the solution. The formula for boiling point elevation is:

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

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

### Step-by-Step Solution:

1. **Identify the van 't Hoff factor (i) for each solute:**
- **NaCl**: Dissociates into Na⁺ and Cl⁻, so \(i = 2\).
- **Sucrose**: A non-electrolyte that does not dissociate, so \(i = 1\).
- **BaCl₂**: Dissociates into Ba²⁺ and 2 Cl⁻ ions, so \(i = 3\).
- **Glucose**: A non-electrolyte that does not dissociate, so \(i = 1\).

2. **Compare the van 't Hoff factors:**
- NaCl: \(i = 2\)
- Sucrose: \(i = 1\)
- BaCl₂: \(i = 3\)
- Glucose: \(i = 1\)

3. **Determine which solute has the highest boiling point elevation:**
- The boiling point elevation is directly proportional to the van 't Hoff factor. Therefore, the higher the value of \(i\), the greater the boiling point elevation.
- Among the solutes, BaCl₂ has the highest \(i\) value of 3.

4. **Conclusion:**
- Since BaCl₂ has the highest van 't Hoff factor, it will produce the highest boiling point elevation at 1 atm pressure.

### Final Answer:
**BaCl₂ will have the highest boiling point at 1 atm pressure.**