Which of the following equation correctly represents molar mass of a solute by knowing boiling point…

Which of the following equation correctly represents molar mass of a solute by knowing boiling point elevation?
  1. $\mathrm{M}_2=\frac{1000 \times \Delta \mathrm{T}_{\mathrm{b}} \times \mathrm{W}_2}{\mathrm{~K}_{\mathrm{b}} \times \mathrm{W}_{\mathrm{i}}}$
  2. $\mathrm{M}_2=\frac{1000 \times \mathrm{K}_{\mathrm{b}} \times \mathrm{W}_1}{\Delta \mathrm{~T}_{\mathrm{b}} \times \mathrm{W}_2}$
  3. $\mathrm{M}_2=\frac{1000 \times \Delta \mathrm{T}_{\mathrm{b}} \times \mathrm{W}_1}{\mathrm{~K}_{\mathrm{b}} \times \mathrm{W}_2}$
  4. $\mathrm{M}_2=\frac{1000 \times \mathrm{K}_{\mathrm{b}} \times \mathrm{W}_2}{\Delta \mathrm{~T}_{\mathrm{b}} \times \mathrm{W}_1}$

Solution

The correct relation between elevation of boiling point $\left(\Delta \mathrm{T}_{\mathrm{b}}\right)$ and molar mass of solute $\left(\mathrm{M}_2\right)$ is $\mathrm{M}_2=\frac{\mathrm{K}_{\mathrm{b}} \times \mathrm{W}_2}{\Delta \mathrm{~T}_{\mathrm{b}} \times \mathrm{W}_1}$ Here, $W_1$ and $W_2$ represents masses of solvent and solute respectively. $K_b$ represents molal elevation in boiling point constant.

Asked in: MHT CET 2024 (03 May Shift 2)

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