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(C) To store an aqueous solution of $CuSO_4$,the metal of the container must not react with $Cu^{2+}$ ions. $A$ reaction will occur if the reduction p

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$Ag$

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(C) To store an aqueous solution of $CuSO_4$,the metal of the container must not react with $Cu^{2+}$ ions. $A$ reaction will occur if the reduction potential of the container metal is lower than that of $Cu^{2+}/Cu$ $(0.34 \ V)$. The reduction potentials $(E^0_{M^{n+}/M})$ are: $E^0_{Fe^{2+}/Fe} = -0.44 \ V$ $E^0_{Ni^{2+}/Ni} = -0.25 \ V$ $E^0_{Al^{3+}/Al} = -1.66 \ V$ $E^0_{Ag^{+}/Ag} = 0.80 \ V$ For the reaction $M + Cu^{2+} \rightarrow M^{n+} + Cu$ to be non-spontaneous,the $E^0_{cell}$ must be negative. $E^0_{cell} = E^0_{cathode} - E^0_{anode} = E^0_{Cu^{2+}/Cu} - E^0_{M^{n+}/M}$. For $E^0_{cell}  E^0_{Cu^{2+}/Cu}$. Comparing values,only $Ag$ has a reduction potential $(0.80 \ V)$ greater than $Cu$ $(0.34 \ V)$. Therefore,$CuSO_4$ can be stored in an $Ag$ container.

In which metal container can an aqueous solution of $CuSO_4$ be stored?
$E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$

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In which metal container can an aqueous solution of $CuSO_4$ be stored? $E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$