The freezing point (in ${}^{\circ}C$) of a solution containing $0.1 \ g$ of $K_3[Fe(CN)_6]$ (Mol. Wt. $329$) in $100 \ g$ of water $(K_f = 1.86 \ K \ kg \ mol^{-1})$ is

For a $0.25 \ m$ solution of $SrCl_2$,the van't Hoff factor is found to be $2.5$. What will be the effective molality of the solution in $m$?

When $9.45 \text{ g}$ of $ClCH_2COOH$ is added to $500 \text{ mL}$ of water,its freezing point drops by $0.5^\circ \text{C}$. The dissociation constant of $ClCH_2COOH$ is $x \times 10^{-3}$. The value of $x$ is ............... (Rounded off to the nearest integer) $[K_{f(H_2O)} = 1.86 \text{ K kg mol}^{-1}]$

At a certain temperature,the vapour pressure of pure water is $76 \ mm$ of $Hg$. When $1 \ mol$ of $Na_2SO_4$ is dissolved in $36 \ mL$ of water,the vapour pressure of the solution becomes $38 \ mm$ of $Hg$. What is the percentage dissociation of $Na_2SO_4$ in the solution?

Which of the following solutions has an osmotic pressure nearest to that of an equimolar solution of $K_4[Fe(CN)_6]$?

Which of the following $0.05 \ M$ aqueous solution will have the lowest freezing point?