We cannot store $CuSO_4$ solution in an iron vessel. Why?

Copper is above iron in the electrochemical series.

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Copper is not in the electrochemical series.

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Copper is more electropositive than iron.

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Iron is above copper in the electrochemical series.

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Solution

The correct option is C. Iron is above copper in the electrochemical series.
Iron is above copper in the electrochemical series and is thus more electropositive than copper. So, iron displaces copper from copper sulphate solution. This liberated copper appears in the form of a red precipitate. Hence, $C u S O_{4}$ solution cannot be stored in an iron vessel.

$F e + C u S O_{4} \to F e S O_{4} + C u$

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