A solution is prepared by dissolving 9.25 g of non volatile solute in 450 ml of water. It has an osmotic pressure of 350 mm of Hg at `27^(@)C`. Assuming the solute is non-electrolyte, determine its molecular mass.
(R = 0.0821 lit atm `K^(-1)mol^(-1)`)

Explanation

To determine the molecular mass of the non-volatile solute, we can follow these steps:

### Step 1: Convert the osmotic pressure from mm of Hg to atm
The osmotic pressure (π) is given as 350 mm of Hg. To convert this to atm, we use the conversion factor:
\[ \text{Pressure in atm} = \frac{\text{Pressure in mm of Hg}}{760} \]
Calculating this gives:
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