$A$ $0.1 \ mol$ of a binary electrolyte undergoes complete dissociation in $250 \ g$ of a protic solvent. If the elevation in boiling point is $1.5 \ K$,the molal elevation constant $(K_b)$ is ............. $K \ kg \ mol^{-1}$.

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

Assuming $100\%$ dissociation of $1 \ m$ $KCl$ solution in water,the freezing point of the solution will be ........ $^oC$. $(K_f = 1.86 \ K \ kg \ mol^{-1})$

$12.25 \ g$ of $CH_3CH_2CHClCOOH$ is added to $250 \ g$ of water to make a solution. If the dissociation constant of the above acid is $1.44 \times 10^{-3}$,the depression in the freezing point of water in $^{\circ}C$ is ($K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$)

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 of the following solutions will have the highest boiling point?