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

The degree of dissociation of $Ca(NO_3)_2$ in a dilute aqueous solution containing $7 \ g$ of the salt per $100 \ g$ of water at $100^{\circ}C$ is $70$ percent. If the vapour pressure of water at $100^{\circ}C$ is $760 \ mm \ Hg$,calculate the vapour pressure of the solution.

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

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 $......... \, ^{\circ}C$.

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

At higher altitude,the boiling point of water is $95\,^oC$. The amount of $NaCl$ added to $1\, kg$ of water $(K_b = 0.52\, K\, kg\, mol^{-1})$ in order to raise the boiling point of the solution to $100\,^oC$ is ......... $g$. (Assuming $90\%$ ionization of $NaCl$)