$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \%$ ionised. The freezing point of this solution is .......... $^oC$. ($K_f = 1.86 \, K \cdot kg \cdot mol^{-1}$ for water) :-

The osmotic pressure of a dilute solution of an ionic compound $XY$ in water is four times that of a solution of $0.01\, M\, BaCl_2$ in water. Assuming complete dissociation of the given ionic compounds in water,the concentration of $XY$ (in $mol\, L^{-1}$) in solution is

If $BaCl_2$ ionizes to an extent of $80 \%$ in aqueous solution, the value of van't Hoff factor is

$A$ solution containing $0.85 \ g$ of $ZnCl_2$ in $125.0 \ g$ of water freezes at $-0.23 \ ^\circ C$. The apparent degree of dissociation of the salt is ($K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$,atomic mass: $Zn = 65.3$ and $Cl = 35.5$)

If $A_2 B$ is $30 \%$ ionised in an aqueous solution,then the value of van't Hoff factor $(i)$ is $............ \times 10^{-1}$.

The measured osmotic pressure of a solution prepared by dissolving $17.4 \ mg$ of $K_2SO_4$ in $2 \ L$ of water at $27^{\circ} C$ is $3.735 \times 10^{-3} \ bar$. The van't Hoff factor is $(R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$; atomic weights $K = 39, S = 32, O = 16)$.