Assuming $100\%$ dissociation of $1 \ m$ $KCl$ solution in water,the freezing point of the solution will be ........ $^oC$. $(K_f = 1.86 \ K \ kg \ mol^{-1})$

$MX_{2}$ dissociates into $M^{2+}$ and $X^{-}$ ions in an aqueous solution,with a degree of dissociation $(\alpha)$ of $0.5$. The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is

The elevation in boiling point of a solution of $13.44 \ g$ of $CuCl_2$ in $1 \ kg$ of water using the following information will be (Molecular weight of $CuCl_2 = 134.4 \ g \ mol^{-1}$ and $K_b = 0.52 \ K \ kg \ mol^{-1}$)

Which of the following $0.1 \, M$ aqueous solutions has the lowest freezing point?

$A$ $0.0020 \ m$ aqueous solution of an ionic compound $[Co(NH_3)_5(NO_2)]Cl$ freezes at $-0.00732 \ ^oC.$ Number of moles of ions which $1 \ mol$ of ionic compound produces on being dissolved in water will be
$(K_f = 1.86 \ ^oC/m)$

$0.5$ molal 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 $........ K$.