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

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

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.

A solution of sucrose (molar mass = 342 g mol^$$-$$) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be (K_f for water = 1.86 K kg mol^$$-$$1)