The properties which depend on the number of solute particles irrespective of their nature relative to the total number of particles in the solution are called colligative properties. These are relative lowering of vapour pressure of the solvent, depression of freezing point of the solvent, elevation of boiling point of the solvent and osmotic pressure of the solution. All of these properties help in calculating the observed molar mass of the solute.
Determination of osmotic pressure is considered best for the determination of molecular mass of the solute.
A 1 litre solution of glucose containing 36 g of it has an osmotic pressure of 4.98 bar at 300 K .
At the same temperature, the osmotic pressure of the solution is 1.52 bar.
The concentration of the solution at 1.52 bar is :

1. A \(0.0610 mol l ^{-1}\)
2. B \(10.9 mol l ^{-1}\)
3. C \(1.6 mol l ^{-1}\)
4. D \(0.00610 mol l ^{-1}\)