The standard reduction potentials of Cu^{2+}, | vedclass

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(D) solution can be stored in a metal vessel if the metal of the vessel does not act as a reducing agent for the metal ions in the solution. This mean

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$CuSO_4$ solution in a silver vessel

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(D) solution can be stored in a metal vessel if the metal of the vessel does not act as a reducing agent for the metal ions in the solution. This means the standard reduction potential of the metal vessel $(E^{o}_{vessel})$ must be greater than the standard reduction potential of the metal ion in the solution $(E^{o}_{ion})$,so that $E^{o}_{cell} = E^{o}_{cathode} - E^{o}_{anode}$ is negative,indicating a non-spontaneous reaction.Given standard reduction potentials $(E^{o})$:$E^{o}_{Zn^{2+}/Zn} = -0.76 \ V$$E^{o}_{Sn^{2+}/Sn} = -0.14 \ V$$E^{o}_{Cu^{2+}/Cu} = 0.34 \ V$$E^{o}_{Ag^{+}/Ag} = 0.80 \ V$Evaluating the options:$A$. $CuSO_4$ in $Zn$: $E^{o}_{Zn} $B$. $AgNO_3$ in $Zn$: $E^{o}_{Zn} $C$. $AgNO_3$ in $Sn$: $E^{o}_{Sn} $D$. $CuSO_4$ in $Ag$: $E^{o}_{Ag} > E^{o}_{Cu}$,no reaction occurs ($Ag + Cu^{2+} \rightarrow$ No reaction).Therefore,$CuSO_4$ solution can be stored in a silver vessel.

The standard reduction potentials of $Cu^{2+}$,$Zn^{2+}$,$Sn^{2+}$ and $Ag^{+}$ are $0.34 \ V$,$-0.76 \ V$,$-0.14 \ V$ and $0.80 \ V$ respectively. Which of the following solutions can be stored in the given vessel without any reaction occurring (under standard conditions)?

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