The freezing point of nitrobenzene is `3^(@)C`. When 1.2 g of chloroform (mol. Wt. =120) is dissolved in 100 g of nitrobenzene, freezing point will be `2.3^(@)C`. When 0.6 g of acetic acid is dissolved in 100 g of nitrobenzene, freezing point of solution is `2.64^(@)C`. If the formula of acetic acid is `(CH_(2)O)_(n)`, find the value of n.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Calculate the depression in freezing point (ΔTf) for chloroform.
The initial freezing point of nitrobenzene is 3°C, and the freezing point after adding chloroform is 2.3°C.

\[ \Delta T_f = T_f^{\text{initial}} - T_f^{\text{final}} = 3°C - 2.3°C = 0.7°C \]
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