Calculate the number of moles of nonvolatile solute dissolved in $0.3 \ kg$ solvent if $\Delta T_{b}=0.3 \ K$ and $K_{b}$ for solvent is $1.8 \ K \ kg \ mol^{-1}$.

To observe an elevation of boiling point of $0.05^{\circ} C$, the amount of a solute (mol. wt. $= 100$) to be added to $100 \ g$ of water $(K_{b} = 0.5)$ is (in $g$)

When common salt is dissolved in water,

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

$1 \ g$ of non-volatile non-electrolyte solute is dissolved in $100 \ g$ of two different solvents $A$ and $B$ whose ebullioscopic constants are in the ratio of $1 : 5$. The ratio of the elevation in their boiling points,$\frac{\Delta T_b (A)}{\Delta T_b (B)}$ is

Arrange the following solutions in order of their increasing boiling points.
$(i) \ 10^{-4} \ M \ NaCl$ $(ii) \ 10^{-4} \ M \ \text{Urea}$ $(iii) \ 10^{-3} \ M \ NaCl$ $(iv) \ 10^{-2} \ M \ NaCl$