$A$ solution containing $2.5 \times 10^{-3} \ kg$ of a solute dissolved in $75 \times 10^{-3} \ kg$ of water boils at $373.535 \ K$. The molar mass of the solute is $..... \ g \ mol^{-1}$. [nearest integer] (Given: $K_b(H_2O) = 0.52 \ K \ kg \ mol^{-1}$,boiling point of water $= 373.15 \ K$)

Sea water contains $29.25\%$ $NaCl$ and $19\%$ $MgCl_2$ by weight of solution. The normal boiling point of the sea water is $..........{}^{\circ}C$ (Nearest integer).
Assume $100\%$ ionization for both $NaCl$ and $MgCl_2$.
Given: $K_b(H_2O) = 0.52 \, K \, kg \, mol^{-1}$.
Molar mass of $NaCl$ and $MgCl_2$ is $58.5$ and $95 \, g \, mol^{-1}$ respectively.

The boiling point of water $(100\,^{\circ}C)$ becomes $100.52\,^{\circ}C$,if $3\,g$ of a non-volatile solute is dissolved in $200\,mL$ of water. The molecular weight of the solute is: (${K_b}$ for water is $0.6\,K\,kg\,mol^{-1}$)

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

Which of the following statements is correct for the boiling point of a liquid?

$A$ solution containing $2 \ g$ of a non-volatile solute in $20 \ g$ of water boils at $373.52 \ K$. The molecular mass of the solute is $....... \ g \ mol^{-1}$. (Nearest integer) Given,water boils at $373 \ K$,$K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$.