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Standard electrode potential data are useful for understanding the suitablilty of an oxidant in a redox titration. Some half cell reactions and their standard potentials are given below:
\( P \)
\[
\begin{array}{l}
\mathrm{MnO}_{4}^{-}(\mathrm{aq})+8 \mathrm{H}^{+}(\mathrm{aq})+5 \mathrm{e}^{-} \longrightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(l) ; \mathrm{E}^{\circ}=1.51 \mathrm{~V} \\
\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})+14 \mathrm{H}^{+}(\mathrm{aq})+6 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Cr}^{3+}(\mathrm{aq})+7 \mathrm{H}_{2} \mathrm{O}(l) ; \mathrm{E}^{\circ}=1.38 \mathrm{~V} \\
\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{e}^{-} \longrightarrow \mathrm{Fe}^{2+}(\mathrm{aq}) ; \mathrm{E}^{\circ}=0.77 \mathrm{~V} \\
\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Cl}^{-}(\mathrm{aq}) ; \mathrm{E}^{\circ}=1.40 \mathrm{~V}
\end{array}
\]
W.
- Identify the only incorrect statement regarding quantitative estimation of aqueous \( \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2} \)
- (A) \( \mathrm{MnO}_{4}^{-} \)can be used in aqueous \( \mathrm{HCl} \)
(B) \( \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \) can be used in aqueous \( \mathrm{HCl} \)
- (C) \( \mathrm{MnO}_{4}^{-} \)can be used in aqueous \( \mathrm{H}_{2} \mathrm{SO}_{4} \)
(D) \( \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-} \) can be used in aqueous \( \mathrm{H}_{2} \mathrm{SO}_{4} \)
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