Question

Can you store copper sulphate solutions in a zinc pot?

Answer 1

\[\ce{E^\circ_{{Zn^{2+}/{ Zn}}}}\] = −0.76 V

\[\ce{E^\circ_{{Cu^{2+}/{ Cu}}}}\] = 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:

Zn | Zn²⁺ || Cu²⁺ | Cu

\[\ce{E^\circ_{cell} = E^\circ_{Cu^{2+}/Cu} - E^\circ_{Zn^{2+}/ Zn}}\]

= 0.34 V – (–0.76 V)

= 1.1 V

Since \[\ce{E^\circ_{cell}}\] is positive, the reaction takes place, and we cannot store CuSO₄ solution in a zinc pot.