What is the expected value of $\Delta T_f$ for $1.25 \ m$ $CaCl_2$ solution if $1.25 \ m$ sucrose solution has $\Delta T_f$ value $x \ K$?

The relative lowering of vapour pressure for $0.1 \ M$ aqueous solutions of $NaCl$,$CuSO_4$,and $K_2SO_4$ is in the ratio of...

The freezing point of a $0.0020 \ m$ aqueous solution of $[CO(NH_3)_5(NO_2)]$ is $-0.00732 \ ^oC$. The number of ions produced (van't Hoff factor,$i$) when $1 \ mol$ of this ionic compound is dissolved in water is ..... $(K_f = 1.86 \ K \ kg \ mol^{-1})$

$AB_2$ is $10\%$ dissociated in water to $A^{2+}$ and $B^{-}$. The boiling point of a $10.0 \text{ molal}$ aqueous solution of $AB_2$ is . . . . . . $^\circ C$. (Round off to the Nearest Integer). [Given: Molal elevation constant of water $K_b = 0.5 \text{ K kg mol}^{-1}$,boiling point of pure water $= 100^\circ C$]

$12.25 \ g$ of $CH_3CH_2CHClCOOH$ is added to $250 \ g$ of water to make a solution. If the dissociation constant of the above acid is $1.44 \times 10^{-3}$,the depression in the freezing point of water in $^{\circ}C$ is ($K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$)

Maximum depression in freezing point is caused by