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 molal elevation constant of water is $0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar is dissolved in $200 \ g$ of water,at what temperature $(^oC)$ will the solution start to boil under $1 \ bar$ pressure?

When a substance is dissolved in a solvent,the vapour pressure of the solvent is decreased. This results in:

Two different solutions were prepared by dissolving sucrose in water having concentrations of $1 \ m$ and $2 \ m$ respectively. The value of $(T_2 - T_1)$ will be ........... $K$. (Given: $K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$)

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? $(K_b = 3.28 \ \text{K kg mol}^{-1})$

Calculate $\Delta T_b$ of a $0.45 \text{ m}$ solution of a nonvolatile solute in a solvent if the molal elevation constant of the solvent is $3.0 \text{ K kg mol}^{-1}$. (in $\text{ K}$)