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

An aqueous solution is prepared by dissolving $0.1 \ mol$ of an ionic salt in $1.8 \ kg$ of water at $35^{\circ} C$. The salt remains $90 \%$ dissociated in the solution. The vapour pressure of the solution is $59.724 \ mm \ Hg$. Vapor pressure of water at $35^{\circ} C$ is $60.000 \ mm \ Hg$. The number of ions present per formula unit of the ionic salt is . . . . . .

When $10^{-3} \ M$ solution of glucose in water freezes at $-0.0186^{\circ} C$,then at what temperature $10^{-3} \ M$ solution of $NaCl$ will freeze (in $^{\circ} C$)?

For very dilute solutions of $BaCl_2$ $(t_1)$ and $KCl$ $(t_2)$ having the same molarity,what is the correct relationship between their boiling points?

At $25 \ ^oC$,the highest osmotic pressure is exhibited by $0.1 \ M$ solution of

$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \% $ ionised. The freezing point of this solution is .............. $^o C$ (Given ${K_f} = 1.86 \, ^o C/m$ for water)