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Question
Can you store copper sulphate solutions in a zinc pot?
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Solution
\[\ce{E^Θ_{{Zn^{2+}/{ Zn}}}}\] = −0.76 V; \[\ce{E^Θ_{{Cu^{2+}/{ Cu}}}}\] = 0.34 V
We have to check whether the following reaction takes place or not.
\[\ce{Zn_{(s)} + CuSO4_{(aq)} -> ZnSO4_{(aq)} + Cu_{(s)}}\]
The cell can be represented as:
\[\ce{Zn | Zn^{2+} || Cu^{2+} | Cu}\]
\[\ce{E^Θ_{cell} = E^Θ_{{Cu^{2+}/{ Cu}}} - E^Θ_{{Zn^{2+}/{ Zn}}}}\]
= 0.34 V – (–0.76 V)
= 1.1 V
Since \[\ce{E^Θ_{cell}}\] is positive, the reaction takes place, and we cannot store \[\ce{CuSO4}\] solution in a zinc pot.
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