The boiling point of 0.2 , mol , kg^{-1} solu | vedclass

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(C) The elevation in boiling point is given by the formula $\Delta T_{b} = i K_{b} m$,where $i$ is the van't Hoff factor,$K_{b}$ is the ebullioscopic

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$X$ is undergoing dissociation in water.

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(C) The elevation in boiling point is given by the formula $\Delta T_{b} = i K_{b} m$,where $i$ is the van't Hoff factor,$K_{b}$ is the ebullioscopic constant,and $m$ is the molality.Since the solutions are equimolal ($m$ is constant) and the solvent is the same ($K_{b}$ is constant),the elevation in boiling point depends directly on the van't Hoff factor $i$.Given that the boiling point of the solution of $X$ is greater than that of $Y$,it implies that $\Delta T_{b}(X) > \Delta T_{b}(Y)$,which means $i_{X} > i_{Y}$.If $X$ undergoes dissociation,its van't Hoff factor $i$ becomes greater than $1$,leading to a higher boiling point compared to a non-dissociating solute.

The boiling point of $0.2 \, mol \, kg^{-1}$ solution of $X$ in water is greater than equimolal solution of $Y$ in water. Which one of the following statements is true in this case?

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