$17.4\%\, (w/v)$ $K_2SO_4$ $(Mw=174\, g/mol)$ solution at $27\, ^\circ C$ is isotonic to $4\%\, (w/v)\, NaOH$ solution at the same temperature. If $NaOH$ is $100\%$ ionized,what is the $\%$ ionization of $K_2SO_4$ in aqueous solution .......... $\%$.

$A$ solution of $17.1$ $w\%$ of sucrose (molar mass $= 342 \ g \ mol^{-1}$) is isotonic with a $x$ $w\%$ solution of oxalic acid (molar mass $= 90 \ g \ mol^{-1}$). Assume the degree of dissociation of oxalic acid as $0.01$. What is $x$?

The boiling point of $0.01 \, M$ aqueous solutions of sucrose,$NaCl$ and $CaCl_2$ would be

The osmotic pressure $(O.P.)$ of equimolar solutions of $Urea$,$BaCl_2$,and $AlCl_3$ will be in the order:

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