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Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half-cell reactions and their standard potentials are given below ;

MnO4-(aq)+8H+(aq)+5e-⟶Mn2+(aq)+4H2O(l),


\( \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+14 \mathrm{H}^{+}(a q)+6 e^{-} \longrightarrow 2 \mathrm{Cr}^{3+}(a q)+7 \mathrm{H}_{2} \mathrm{O}(l) \)
\( E^{\circ}=1.38 \mathrm{~V} \)
\( \mathrm{Fe}^{3+}(a q)+e^{-} \longrightarrow \mathrm{Fe}^{2+}(a q) \quad E^{\circ}=0.77 \mathrm{~V} \)
\( \mathrm{Cl}_{2}(g)+2 e^{-} \longrightarrow 2 \mathrm{Cl}^{-}(a q) \quad E^{\circ}=1.40 \mathrm{~V} \)
Identify the incorrect statement regarding the 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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