$A$ solution containing $0.1050 \ g$ of a substance in $15.84 \ g$ of ether has a boiling point $1 \ ^\circ C$ higher than that of pure ether. What is the molar mass of the substance? [Given: Molar elevation constant for ether per $100 \ g = 21.6$]

Molal elevation constant is the elevation in boiling point produced by

Calculate the molar mass of a non-volatile solute when $5 \ g$ of it is dissolved in $50 \ g$ of solvent,which boils at $119.6^{\circ} C$. $[K_{b} = 3.2 \ K \ kg \ mol^{-1}$,boiling point of pure solvent $= 118^{\circ} C]$.

The elevation in boiling point for one molal solution of a solute in a solvent is called

When $0.5 \ g$ of anthracene is dissolved in $35 \ g$ of chloroform,the boiling point increases by $0.3 \ K$. If the $K_b$ value for $CHCl_3$ is $3.9 \ K \ kg \ mol^{-1}$,the experimental molar mass of anthracene is ......... $g \ mol^{-1}$.

$5 \text{ g}$ of urea is dissolved in $100 \text{ g}$ of water. Find the amount of glucose to be dissolved in $120 \text{ g}$ of water so that the boiling points of both solutions are the same. [Molar mass of urea $= 60 \text{ g mol}^{-1}$, Molar mass of glucose $= 180 \text{ g mol}^{-1}$] (in $\text{ g}$)