$A$ solution of non-volatile solute has a boiling point elevation of $1.75 \ K$. Calculate the molality of the solution $[K_{b} = 3.5 \ K \ kg \ mol^{-1}]$.

When $10 \ g$ of a non-volatile solute is dissolved in $100 \ g$ of benzene,it raises the boiling point by $1 \ ^{\circ}C$. The molecular mass of the solute is ....... $g \ mol^{-1}$. ($K_b$ for benzene $= 2.53 \ K \ kg \ mol^{-1}$)

The molal elevation boiling point constant for water is $0.513 \ ^{\circ}C \ kg \ mol^{-1}$. Calculate the boiling point of the solution if $0.1 \ mol$ of sugar is dissolved in $200 \ g$ of water. (in $^{\circ}C$)

The molal elevation constant of water is $0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar is dissolved in $200 \ g$ of water,at what temperature $(^oC)$ will the solution start to boil under $1 \ bar$ pressure?

If $K_{b}$ denotes the molal elevation constant of water,then the boiling point of an aqueous solution containing $36 \ g$ of glucose (molar mass $= 180 \ g/mol$) per $1 \ kg$ of water is:

$A$ solution is prepared by dissolving a $2.5 \ g$ sample of an unknown compound in $34 \ g$ of benzene,$C_6H_6$. The solution boils at $1.38 \ ^\circ C$ higher than pure benzene. Which expression gives the molar mass of the unknown compound? $K_b$ of $C_6H_6$ is $2.53 \ ^\circ C \ m^{-1}$.