p_A and p_B are the vapour pressure of pure liquid components, A and B, respectively of an ideal binary solution. If x_A represents the mole fraction of component A, the total pressure of the solution will be

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.