Elevation in boiling point of the aqueous sol | vedclass

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(C) The elevation in boiling point is given by the formula $\Delta T_b = i 	imes K_b 	imes m$. For $0.01 \ M$ urea (a non-electrolyte),the van't Hof

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approximately three times

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(C) The elevation in boiling point is given by the formula $\Delta T_b = i 	imes K_b 	imes m$. For $0.01 \ M$ urea (a non-electrolyte),the van't Hoff factor $i = 1$. For $0.01 \ M \ BaCl_2$ (a strong electrolyte),it dissociates as $BaCl_2 ightarrow Ba^{2+} + 2Cl^-$,so the van't Hoff factor $i = 3$. Since the molality $m$ and the ebullioscopic constant $K_b$ are the same for both solutions,the ratio of elevation in boiling point is $\frac{\Delta T_b(BaCl_2)}{\Delta T_b(	ext{urea})} = \frac{i(BaCl_2)}{i(	ext{urea})} = \frac{3}{1} = 3$. Therefore,the elevation in boiling point of $0.01 \ M \ BaCl_2$ is approximately three times that of $0.01 \ M$ urea.

Elevation in boiling point of the aqueous solution of $0.01 \ M \ BaCl_2$ compared to $0.01 \ M$ urea is . . . . . . .

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