Why is freezing point depression of 0.1 M sodium chloride solution nearly twice that of 0.1 M glucose solution ?

Explanation

To understand why the freezing point depression of a 0.1 M sodium chloride (NaCl) solution is nearly twice that of a 0.1 M glucose solution, we need to analyze the concept of freezing point depression and the behavior of the solutes in the solutions.

### Step-by-Step Solution:

1. **Understanding Freezing Point Depression**:
- Freezing point depression (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. **Dissociation of Sodium Chloride**:
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