0.5 molal aqueous solution of a weak acid is 20% iionized. If `K_f` for water is `1.86K kg mol^-1`. The lowering in freezing point of the solution is

In a 0.2 molal aqueus solution of a weak acid HX the degree of dissociation is 0.25. The freezing point of the solution will be nearest to: ( K_(f)=1.86 K kg "mol"^(-1) ) a) -0.26^(@)C b) 0.465^(@)C c) -0.48^(@)C d) -0.465^(@)C

0.2 m aqueous solution of a weak acid is 20% dissociated. The boiling point of this solution is (K_(b) of water= 0.52Km^-1)

If the freezing point of a 0.01 molal aqueous solution of a cobalt chloride ammonia complex is -0.0558^@C , the number of chloride in the coordination sphere of the complex is [K_f of water =1.86K kg mol^-1]

A 0.1539 molal aqueous solution of cane sugar ( molar mass-342gmol^-1 ) has a freezing of 271K while the freezing point of pure water is 273.15K. What will be the freezing point of an aqueous solution containing 5 g of glucose (mol.mass=180gmol^-1) per 100 g of solution.

The density of 2.0 M solution of solute is 1.2 gm/ml. If the molecular mass of solute is 100 gm "mol"^(-1) then the molality of the solution is

1.5 g of a non-volatile non-electrolyte is dissolved in 50 g of benzene (K_b=2.5K kg mol^-1) . The elevation of boiling point of the solution is 0.75K. The molecular weigth of the solute is gmol^-1 is

31 gm of ethylene glycol (C_2H_6O_2) is mixed with 500 gm of solvent. (K_f = 2 K kg "mol"^(-1)) . What is the freezing point of the solution in K ? (freezing point of solvent = 273K)