0.2 molal acid HX is 20% ionised in solution, `K_(f)=1.86K "molality"^(-1)`. The freezig point of the solution is

0.2 molal aqueous solution of acid HX is 20% ionised. K_f="1.86 K molal"^(-1) . The freezing point of the solution is very close to:

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 :

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 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 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

A 0.2 molar aqueous solution of a weak acid (HX) is 20% ionised . The freezing point of the solution is: (Given: K_(f)=1.86^(@) C kg" "mol^(-1)" for water")