The freezing point of an aqueous solution which contains $5\%$ by mass urea,$1.0\%$ by mass $KCl$,and $10\%$ by mass glucose is ........ $K$. $\left( K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1} \right)$

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution,the change in freezing point of water $(\Delta T_f),$ when $0.01 \ mol$ of sodium sulphate is dissolved in $1 \ kg$ of water,is $(K_f = 1.86 \ K \ kg \ mol^{-1})$ (in $K$).

The correct order of boiling point of the given aqueous solutions is:

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

$0.01 \ M$ 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 osmotic pressure values of $0.1 \ M$ solutions of $KNO_3$ and $CH_3COOH$ are $P_1$ and $P_2$ respectively. Establish the relationship between them.