1 mol each of the following compounds is dis | vedclass

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(D) The elevation in boiling point is given by the formula $\Delta T_b = i 	imes K_b 	imes m$.
Since $1 \ mol$ of each compound is dissolved in $1

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$HI$

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(D) The elevation in boiling point is given by the formula $\Delta T_b = i imes K_b imes m$. Since $1 \ mol$ of each compound is dissolved in $1 \ L$ of solution,the molality $(m)$ is the same for all. Therefore,$\Delta T_b$ is directly proportional to the van't Hoff factor $(i)$. The van't Hoff factor $(i)$ depends on the degree of dissociation $(\alpha)$. Stronger acids dissociate more completely in water. The acid strength order for hydrogen halides is $HI > HBr > HCl > HF$. This is because the bond dissociation energy follows the order $HI < HBr < HCl < HF$. Since $HI$ has the lowest bond dissociation energy,it dissociates most readily,leading to the highest number of ions in the solution. Thus,$i$ is maximum for $HI$,resulting in the largest $\Delta T_b$ value.

$1 \ mol$ each of the following compounds is dissolved in $1 \ L$ of solution. Which will have the largest $\Delta T_b$ value?

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