Question
Can you store copper sulphate solutions in a zinc pot?
✓
Answer
Zn being more reactive than Cu , displaces Cu from $\mathrm{CuSO}_4$ solution as follows: $\mathrm{Zn}(\mathrm{s})+\mathrm{CuSO}_4(\mathrm{aq}) \rightarrow \mathrm{ZnSO}_4(\mathrm{ag})+\mathrm{Cu}(\mathrm{s})$
In terms of EMF, we have
$Zn|Zn^{2+}||Cu^{2+}|Cu$
$\text{E}^\circ_\text{cell}=\text{E}^\circ_{\text{Cu}^{2+}\text{Cu}}-\text{E}^\circ_{\text{Zn}^{2+}/\text{Zn}}$
$= 0.34\ V - (-0.76\ V)$
$= 1.10\ V$
As $\text{E}^\circ_\text{cell}$ is positive, reaction takes place, i.e., Zn reacts with copper and hence, we cannot store $CuSo_4$ solution in zinc pot.
In terms of EMF, we have
$Zn|Zn^{2+}||Cu^{2+}|Cu$
$\text{E}^\circ_\text{cell}=\text{E}^\circ_{\text{Cu}^{2+}\text{Cu}}-\text{E}^\circ_{\text{Zn}^{2+}/\text{Zn}}$
$= 0.34\ V - (-0.76\ V)$
$= 1.10\ V$
As $\text{E}^\circ_\text{cell}$ is positive, reaction takes place, i.e., Zn reacts with copper and hence, we cannot store $CuSo_4$ solution in zinc pot.
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