$0.01 \ M$ solutions of glucose,phenol,and potassium chloride were prepared in water. The boiling points of these solutions follow the order:

$A$ 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 $K$)

Mark the correct relationship between the boiling points of very dilute solutions of $BaCl_2$ $(t_1)$ and $KCl$ $(t_2)$,having the same molarity.

$1 \ mol$ each of the following compounds is dissolved in $1 \ L$ of solution. Which will have the largest $\Delta T_b$ value?

If $A_2 B$ is $30 \%$ ionised in an aqueous solution,then the value of van't Hoff factor $(i)$ is $............ \times 10^{-1}$.

Which one of the following $0.06 \ M$ aqueous solutions has the lowest freezing point?