Depression in freezing point of solution of electrolytes are generally

Options

A. lower
B. higher than what should be normally
C. low or high depending upon nature of electrolyte
D. what it should be normally

Answer

**Step-by-Step Text Solution:**

1. **Understanding Depression in Freezing Point**:
The depression in freezing point (ΔTf) is a colligative property, which means it depends on the number of solute particles in a solution rather than the identity of the solute.

2. **Formula for Depression in Freezing Point**:
The formula for calculating the depression in freezing point is given by:
\[ \Delta Tf = i \cdot K_f \cdot m \]
where:
- \( \Delta Tf \) = depression in freezing point
- \( i \) = van 't Hoff factor (number of particles the solute splits into)
- \( K_f \) = freezing point depression constant of the solvent
- \( m \) = molality of the solution

3. **Role of the van 't Hoff Factor (i)**:
The van 't Hoff factor (i) varies for different electrolytes. For example, sodium chloride (NaCl) dissociates into two ions (Na⁺ and Cl⁻), so \( i = 2 \). In contrast, a non-electrolyte like glucose does not dissociate, so \( i = 1 \).

4. **Effect of Electrolyte Nature on Depression**:
Since ΔTf is directly proportional to \( i \), the greater the number of ions produced by an electrolyte, the higher the value of \( i \), leading to a greater depression in freezing point. Conversely, if an electrolyte produces fewer ions, the depression in freezing point will be lower.

5. **Conclusion**:
Therefore, the depression in freezing point of solutions of electrolytes can be either lower or higher than expected, depending on the nature of the electrolyte and the number of ions it produces when dissolved.

**Final Answer**: The depression in freezing point of solutions of electrolytes is generally lower or higher depending upon the nature of the electrolyte.

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