If `0.1M` solutions of `K_(4)[Fe(CN)_(6)]` is prepared at `300K` then its density`=1.2gm//mL`. If solute is `50%` dissociated calculate `DeltaP` of solutions if `P` of pure water `=25mm "of" Hg`. `(K=39,Fe=56)`

Explanation

To solve the problem step by step, we will follow the outlined process in the video transcript.

### Step 1: Determine the Van't Hoff factor (i)
The dissociation of \( K_4[Fe(CN)_6] \) can be represented as:
\[ K_4[Fe(CN)_6] \rightarrow 4K^+ + [Fe(CN)_6]^{4-} \]
This means that one formula unit of \( K_4[Fe(CN)_6] \) dissociates into 5 particles (4 potassium ions and 1 complex ion).
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