The molal elevation constant of water is $0.51 \ K \, kg \, mol^{-1}$. The boiling point of $0.1 \ m$ aqueous $NaCl$ solution is nearly .......... $^oC$.

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

The osmotic pressure of equimolar solutions of urea,$BaCl_2$,and $AlCl_3$ will be in the order:

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 $NaCl$)

Which of the following aqueous solutions has the highest boiling point,under identical conditions having a concentration of $0.03 \ m$?

The elevation in the boiling point of an aqueous solution of $NaCl$ is $0.01^{\circ}C$. If its van't Hoff factor is $1.92$,the molality of the $NaCl$ solution is: $(K_{b} \text{ for water} = 0.52 \ K \ kg \ mol^{-1})$ (in $m$)