The molal boiling point constant for water is $0.513 \, ^oC \, kg \, mol^{-1}$. When $0.1 \, mol$ of sugar is dissolved in $200 \, mL$ of water,the solution boils under a pressure of one atmosphere at ......... $^oC$.

Calculate the molality of a solution of a nonvolatile solute having a boiling point elevation of $1.89 \ K$,if the boiling point elevation constant of the solvent is $3.15 \ K \ kg \ mol^{-1}$. (in $m$)

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 salt is dissolved in water,then.....

If the boiling point of a urea solution is $100.18^{\circ}C$ and $K_b$ for water is $0.512 \ K \ kg \ mol^{-1}$,what is the molality of the solution? (Boiling point of water $= 100^{\circ}C$)

$18 \, g$ of glucose $(C_{6}H_{12}O_{6})$ dissolved in $1 \, kg$ of water is heated to boiling. The boiling point (in $K$) measured at $1 \, atm$ pressure is closest to: [Ebullioscopic constant,$K_{b}$ for water is $0.52 \, K \, kg \, mol^{-1}$. Consider the boiling point of pure water to be $373.15 \, K$]