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.

$5 \ g$ of $Na_2SO_4$ was dissolved in $x \ g$ of $H_2O$. The change in freezing point was found to be $3.82 \ ^oC$. If $Na_2SO_4$ is $81.5 \%$ ionised,the value of $x$ ($K_f$ for water $= 1.86 \ ^oC \ kg \ mol^{-1}$) is approximately .............. $g$ (molar mass of $S = 32 \ g \ mol^{-1}$ and that of $Na = 23 \ g \ mol^{-1}$)

Which one of the following $0.10 \ M$ aqueous solutions will exhibit the largest freezing point depression?

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.

If $0.004 \ M \ Na_2SO_4$ and $0.01 \ M$ glucose aqueous solutions are isotonic,then the degree of dissociation of $Na_2SO_4$ is ........ $\%$.

What will be the osmotic pressure in $atm$ of a $0.2 \ M$ $K_4[Fe(CN)_6]$ solution at $27 \ ^oC$?