In a 0.5 molal solution KCl, KCl is 50% dissociated. The freezing point of solution will be (`K_(f)` = 1.86 K kg `mol^(-1)`):

If 0.1 m aqueous solution of calcium phosphate is 80% dissociated then the freezing point of the solution will be (K_f of water = 1.86K kg mol^(-1))

If 0.1 m aqueous solution of calcium phosphate is 80% dissociated then the freezing point of the solution will be ( K_f of water = 1.86K kg mol^(-1))

KBr is 80% dissociated in aqueous solution. The freezing point of a 0.5 molal solution is 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 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) )