If the boiling point of water is $100 \,^{\circ}C$,how many grams of $NaCl$ must be added to $500 \,g$ of water to increase the boiling point by approximately $1 \,^{\circ}C$ (in $,g$)? Given $(K_{b})_{H_2O} = 0.52 \,K \cdot kg/mol$.

When $0.01 \ mol$ of nonvolatile solute is dissolved in a certain solvent,calculate the mass of the solvent in $kg$ if $\Delta T_{b} = 0.6 \ K$ and $K_{b}$ for the solvent $= 2 \ K \ kg \ mol^{-1}$. (in $kg$)

The rise in boiling point of a solution containing $1.8 \ g$ of glucose in $100 \ g$ of solvent is $0.1^{\circ} C$. The molal elevation constant of the liquid is

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)

The correct relation between the elevation in boiling point and the molar mass of a solute is: ($W_1$ and $W_2$ are respectively weight of solvent $\&$ solute)

$180 \ g$ of glucose,$C_6H_{12}O_6$,is dissolved in $1 \ kg$ of water in a vessel. The temperature at which water boils at $1.013 \ bar$ is $ . . . . . . $ (given,$K_b$ for water is $0.52 \ K \ kg \ mol^{-1}$. Boiling point for pure water is $373.15 \ K$) (in $K$)