Consider a titration of potassium dichromate | vedclass

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(D) The formula of Mohr's salt is $(NH_4)_2Fe(SO_4)_2 \cdot 6H_2O$. In this salt,the iron is in the $+2$ oxidation state $(Fe^{2+})$.During the titrat

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$6$

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(D) The formula of Mohr's salt is $(NH_4)_2Fe(SO_4)_2 \cdot 6H_2O$. In this salt,the iron is in the $+2$ oxidation state $(Fe^{2+})$.During the titration with potassium dichromate $(K_2Cr_2O_7)$ in an acidic medium,$Fe^{2+}$ is oxidized to $Fe^{3+}$ and $Cr_2O_7^{2-}$ is reduced to $Cr^{3+}$.The balanced chemical equation is:$Cr_2O_7^{2-} + 14H^+ + 6Fe^{2+} \rightarrow 2Cr^{3+} + 6Fe^{3+} + 7H_2O$From the stoichiometry of the reaction,$1$ mole of dichromate ion reacts with $6$ moles of $Fe^{2+}$ ions.Since each mole of Mohr's salt contains $1$ mole of $Fe^{2+}$,the number of moles of Mohr's salt required per mole of dichromate is $6$.

Consider a titration of potassium dichromate solution with acidified Mohr's salt solution using diphenylamine as an indicator. The number of moles of Mohr's salt required per mole of dichromate is

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