In comparison to a $0.01 \ M$ solution of glucose,the depression in freezing point of a $0.01 \ M \ MgCl_2$ solution is (Molecular weight of $MgCl_2 = 95$,molecular weight of glucose $= 180$).

Between aqueous solutions of $0.01 \ m \ KCl$ and $0.01 \ m \ BaCl_2$ (strong electrolytes),the freezing point of the $KCl$ solution is $-2^{\circ}C$. The freezing point of the $BaCl_2$ solution will be ..... $^{\circ}C$.

When mercuric iodide $(HgI_2)$ is added to an aqueous solution of potassium iodide $(KI)$,the

The freezing point depression constant for water is $1.86 \, ^\circ C \, m^{-1}$. If $5.00 \, g$ of $Na_2SO_4$ is dissolved in $45.0 \, g$ of $H_2O$,the freezing point is changed by $3.82 \, ^\circ C$. Calculate the van't Hoff factor $(i)$ for $Na_2SO_4$.

For a $0.1 \, molal$ aqueous solution of $2-$iodopropanoic acid,the degree of dissociation is $5 \%$. The freezing point of the solution will be ............ $^o C$.

For a $0.1 \ M \ Ba(NO_3)_2$ solution, the van't Hoff factor is $2.74$. The degree of dissociation is .............