A 0.1 molal aqueous solution of a weak acid is 30% ionized. If K_f for water is 1.86^oC/m, the freezing point of the solution will be

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