The freezing points of equimolar solutions of glucose,$KNO_3$ and $AlCl_3$ are in the order of:

The molal elevation constant of water is $0.52 \, ^{\circ}C \, kg \, mol^{-1}$. The boiling point of $1.0 \, m$ aqueous $KCl$ solution (assuming complete dissociation of $KCl$) should be $......... \, ^{\circ}C$.

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

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 . . . . . .

$0.5 \text{ molal}$ aqueous solution of a weak acid $(HX)$ is $20\%$ ionised. If $K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$,the depression in freezing point of the solution is $......... \ K$.

Identify the compound amongst the following whose $0.1 \ M$ aqueous solution has the highest boiling point.