A `0.025 m` solution of monobasic acids has a freezing point of `-0.060^(@)C`. What are `K_(a)` and `pK_(a)` of the acid? `(K_(f)=1.86^(@)C)`

A 0.025 m solution of mono basic acid had a freezing point of 0.06^(@)C . Calculate K_(a) for the acid K_(f) for H_(2)O=1.86^(@) "molality"^(-1) .

A 0.075 molar solution of monobasic acid has a freezing point of -0.18^(@)C . Calculate K_(a) for the acid , (k_(f)=1.86)

A 0.075 molal solution of monobasic acid has a freezing point of -0.18^(@)C . Calculate K_(a) for the acid , (k_(f)=1.86)

A 0.1 molal solution of an acid is 4.5% ionized. Calculate freezing point. (molecular weight of the acid is 300 ). K_(f)="1.86 K mol"^(-1)"kg".

A 0.1 molal solution of an acid is 4.5% ionized. Calculate freezing point. (molecular weight of the acid is 300 ). K_(f)="1.86 K mol"^(-1)"kg".

A 0.2 molal aqueous solution of weak acid (HX) is 20% ionised. The freezing point of this solution is (Given, K_(f) = 1.86^(@) C m^(-1) for water)