Calculate the boiling point elevation of a solution if $15 \ g$ of urea is dissolved in $1000 \ g$ of water. $\left[K_{b} \text{ for water} = 0.52 \ K \ kg \ mol^{-1}; \text{ molar mass of urea} = 60 \ g \ mol^{-1}\right]$ (in $K$)

When a substance is dissolved in a solvent,the vapour pressure of the solvent decreases. It brings:

Which of the following solutions will exhibit the highest boiling point?

The molality of an aqueous dilute solution containing a non-volatile solute is $0.1 \ m$. What is the boiling temperature (in $^{\circ}C$) of the solution? (Boiling point elevation constant,$K_b = 0.52 \ K \ kg \ mol^{-1}$; boiling temperature of water $= 100^{\circ}C$).

The boiling point of a solution of $0.11 \ g$ of a substance in $15 \ g$ of ether was found to be $0.1 \ ^\circ C$ higher than that of the pure ether. The molecular weight of the substance will be $(K_b = 2.16 \ K \ kg \ mol^{-1})$.

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