An iron wire is immersed in a solution containing $Z n S O_{4}$ and $N i S O_{4}$ . Predict giving reasons which of the following reactions is likely to proceed?
(i) Iron reduces $Z n^{2 +}$ ions (ii) Iron reduces $N i^{2 +}$ ions.
Given: $E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 v o l t; E_{F e^{2 +} / F e}^{\circ} = - 0.44 v o l t$ and $E_{N i^{2 +} / N i}^{\circ} = - 0.25 v o l t$ .

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Solution

$\to$ When iron is immersed in $Z n S O_{4}$ , no reaction will occur as iron is less reactive than $Z n^{2 +}$ and cannot displace $Z n^{2 +}$ from $Z n S O_{4}$ .
$\to$ When iron is immersed in $N i S O_{4}$ , it will displace $N i^{2 +}$ from $N i S O_{4}$ and form $F e S O_{4}$ , because $F e^{2 +}$ is more reactive and has reduction potential less than $N i^{2 +}$ and hence iron oxidises & displaces $N i^{2 +}$ from $N i S O_{4}$

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