$0.15 \ g$ of a solute is dissolved in $15 \ g$ of a solvent. If the solution boils at a temperature $0.215 \ K$ higher than the boiling point of the pure solvent,what is the molar mass of the solute? $(K_b = 2.15 \ K \ kg \ mol^{-1})$

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

$2 \, g$ of a non-volatile non-electrolyte solute is dissolved in $200 \, g$ of two different solvents $A$ and $B$ whose ebullioscopic constants are in the ratio of $1: 8$. The elevation in boiling points of $A$ and $B$ are in the ratio $\frac{x}{y} (x: y)$. The value of $y$ is .... (Nearest integer)

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 $= 100^{\circ}C$).

Molal elevation constant is the elevation in boiling point produced by

When $3.3 \ g$ of an unknown substance is dissolved in $125 \ g$ of benzene (boiling point $80^\circ \text{C}$),the boiling point of the resulting solution is $80.66^\circ \text{C}$. What is the molar mass of the unknown substance? $(K_b = 3.28 \ \text{K kg mol}^{-1})$