`0.6 mL` of acetic acid `(CH_(3)COOH)` having density `1.06 g mL^(-1)` is dissolved in `1 L` of water. The depression in freezing point observed for this strength of acid was `0.0205^(@)C`.Calculate the Van't Hoff factor and dissociation constant of the acid. `K_(f)` for `H_(2)O=1.86 K kg ^(-1) "mol"^(-1))`

Explanation

To solve the problem, we need to calculate the Van't Hoff factor (i) and the dissociation constant (K) of acetic acid (CH₃COOH). Here's a step-by-step breakdown of the solution:

### Step 1: Calculate the mass of acetic acid
Given:
- Volume of acetic acid = 0.6 mL
- Density of acetic acid = 1.06 g/mL

Using the formula:
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