When common salt is dissolved in water,

Which of the following aqueous solutions will have a boiling point of $102.2^{\circ} C$? The molal elevation constant for water is $K_b = 0.512 \ K \ kg \ mol^{-1}$. (Note: The provided constant $2.2 \ K \ kg \ mol^{-1}$ in the prompt is incorrect for water; using standard $K_b = 0.512 \ K \ kg \ mol^{-1}$ for calculation).

The elevation in boiling point of a solution containing $1.8 \ g$ of glucose in $100 \ g$ of solvent is $0.1^{\circ}C$. The value of $K_b$ for the solvent is ........ $\frac{K}{m}$.

If the boiling points of two solvents $X$ and $Y$ (having same molecular weights) are in the ratio $2 : 1$ and their enthalpies of vaporization are in the ratio $1 : 2$,then the boiling point elevation constant of $X$ is $\underline{ m }$ times the boiling point elevation constant of $Y$. The value of $m$ is $.....$. (Nearest integer)

$1 \ g$ of non-volatile non-electrolyte solute is dissolved in $100 \ g$ of two different solvents $A$ and $B$ whose ebullioscopic constants are in the ratio of $1 : 5$. The ratio of the elevation in their boiling points,$\frac{\Delta T_b (A)}{\Delta T_b (B)}$ is

The molal elevation constant is the ratio of the elevation in boiling point to the $......$.