$13.44 \ g$ of $CuCl_2$ is dissolved in $1 \ kg$ of water. Determine the elevation in boiling point of the solution. [$K_b = 0.52 \ K \ kg \ mol^{-1}$,$mol \ wt$ of $CuCl_2 = 134.4$]

Calculate the molality of a solution of a nonvolatile solute having a boiling point elevation of $1.89 \ K$,if the boiling point elevation constant of the solvent is $3.15 \ K \ kg \ mol^{-1}$. (in $m$)

When a substance is dissolved in a solvent,the vapour pressure of the solvent is decreased. This results in:

Which of the following formulas correctly gives the value of the ebullioscopic constant $(K_{b})$?

Calculate the boiling point of an aqueous solution containing $18 \text{ g}$ of glucose in $100 \text{ g}$ of water, given that the molal elevation constant $(K_b)$ of water is $0.5 \text{ K kg mol}^{-1}$. [Molar mass of glucose $= 180 \text{ g mol}^{-1}$ and boiling point of pure water $= 100^{\circ}\text{C}$] (in $^{\circ}\text{C}$)

$180 \ g$ 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 $K$)