The freezing point of solution containing `0.2 g` of acetic acid in `20.0 g` of benzene is lowered by `0.45^(@)C`. Calculate the degree of association of acetic acid in benzene.
`(K_(f)=5.12 K^(@) mol^(-1) kg^(-1))`

Explanation

To solve the problem, we will follow these steps:

### Step 1: Identify the given data
- Mass of acetic acid (w2) = 0.2 g
- Mass of benzene (w1) = 20.0 g
- Freezing point depression (ΔTf) = 0.45 °C
- Freezing point depression constant for benzene (Kf) = 5.12 K kg⁻¹ mol⁻¹

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