A `0.1` molal aqueous solution of a weak acid is `30%` ionized. If `K_(f)` for water is `1.86^(@)C//m`, the freezing point of the solution will be.

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

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86K kg mol^(-1) , the lowering in freezing point of the solution is

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86K kg mol^(-1) , the lowering in freezing point of the solution is

0.5 molar aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) for water is 1.86 K kg mol^(-1) , the lowering in freezing point of the solution is

0.5 molal aqueous solution of a weak acid (HX) is 20% ionised. If K_(f) of water is 1.86 K kg "mol"^(-1) , the lowering in freezing point of the solution is :

In a 0.2 molal aqueous solution of a weak acid HX the degree of ionization is 0.3. Taking K_(f) for water as 1.85, the freezing point of the solution will be nearest to