$A$ 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 $x$?

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 $K$).

An aqueous solution of a salt $MX_2$ at a certain temperature has a van't Hoff factor of $2$. The degree of dissociation for this solution of the salt is

$0.004 \ M \ K_2SO_4$ solution is isotonic with $0.01 \ M$ glucose solution. The percentage dissociation of $K_2SO_4$ is $........$ (Nearest integer).

The Van't Hoff factor of $Ca(NO_3)_2$ is

$A$ sample of water is found to contain $5.85 \% \left(\frac{w}{w}\right)$ of $AB$ (molecular mass $58.5$) and $9.50 \% \left(\frac{w}{w}\right)$ $XY_2$ (molecular mass $95$). Assuming $80 \%$ ionisation of $AB$ and $60 \%$ ionisation of $XY_2$, the freezing point of the water sample is: [Given, $K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$, freezing point of pure water $= 273 \ K$ and $A, B, X, Y$ are monovalent ions.] (in $K$)