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(B) The molar mass of $FeSO_4$ is $56 + 32 + 4 	imes 16 = 152 \ g/mol$. Given experimental molecular mass $(M_{exp})$ = $80 \ g/mol$. The van't Hoff

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$0.9$

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(B) The molar mass of $FeSO_4$ is $56 + 32 + 4 	imes 16 = 152 \ g/mol$. Given experimental molecular mass $(M_{exp})$ = $80 \ g/mol$. The van't Hoff factor $(i)$ is calculated as $i = \frac{M_{theoretical}}{M_{experimental}} = \frac{152}{80} = 1.9$. For the dissociation of $FeSO_4 ightleftharpoons Fe^{2+} + SO_4^{2-}$, the number of ions produced $(n)$ is $2$. The degree of dissociation $(\alpha)$ is given by the formula $\alpha = \frac{i - 1}{n - 1}$. Substituting the values: $\alpha = \frac{1.9 - 1}{2 - 1} = \frac{0.9}{1} = 0.9$.

For an aqueous solution of $FeSO_4$, the experimental molecular mass is found to be $80 \ g/mol$. What is the degree of dissociation of the salt?

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