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 $100\,^oC$ (assume $90\%$ ionisation of $NaCl$) is .......... $g$.

We have three aqueous solutions of $NaCl$ labelled as '$A$','$B$' and '$C$' with concentrations $0.1 \ M$,$0.01 \ M$,and $0.001 \ M$ respectively. The value of the Van't Hoff factor for these solutions will be in the order . . . . . . .

In which case is Raoult's law not applicable?

$AB_2$ is $10\%$ dissociated in water to $A^{2+}$ and $B^{-}$. The boiling point of a $10.0 \text{ molal}$ aqueous solution of $AB_2$ is . . . . . . $^\circ C$. (Round off to the Nearest Integer). [Given: Molal elevation constant of water $K_b = 0.5 \text{ K kg mol}^{-1}$,boiling point of pure water $= 100^\circ C$]

$0.01 \ M$ solutions of $KCl$ and $BaCl_2$ are prepared in water. The freezing point of $KCl$ is found to be $-2 \ ^oC$. What is the freezing point of $BaCl_2$ if it is completely ionised? ............. $^oC$

The $\Delta T_{b}$ value for $0.01 \ m$ $KCl$ solution is $0.01 \ K$. What is the Van't Hoff factor? $(K_{b}$ for water $= 0.52 \ K \ kg \ mol^{-1})$