In a `0.2` molal aqueous solution of weak acid `HX` (the degree of dissociation `0.3`) the freezing point is (given `K_(f) = 1.85 K molality^(-1)`):

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

In a 2.0 molal aqueus solution of a weak acid HX the degree of disssociation is 0.25. The freezing point of the solution will be nearest to: ( K_(f)=1.86 K kg "mol"^(-1) )

In a 2.0 molal aqueus solution of a weak acid HX the degree of disssociation is 0.25. The freezing point of the solution will be nearest to: ( K_(f)=1.86 K kg "mol"^(-1) )

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

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

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-

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-

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-