200 mL of an aqueous solution of a protein contains its 1.26 g. The osmotic pressure of this solution at 300 K is found to be 2.57 $$ \times $$ 10^$$-$$3 bar. The molar mass of protein will be (R = 0.083 L bar mol^$$-$$1 K^$$-$$1)

The freezing point depression constant for water is $$-$$1.86^o C m^$$-$$1. If 5.00 g Na₂SO₄ is dissolved in 45.0 g H₂O, the freezing point is changed by $$-$$3.82^oC. Calculate the van't Hoff factor for Na₂SO₄.

The van't Hoff factor $$i$$ for a compound which undergoes dissociation in one solvent and association in other solvent is respectively

An aqueous solution is 1.00 molal in KI. Which change will cause the vapour pressure of the solution to increase?