Question

Explain why putting copper (II) metal in a solution of iron (II) sulphate doesn't displace the iron (II) cations from solution.

Answer 1

Copper (II) sulphate reacts with Iron (II) sulphate according to the equation below;

$2FeSO_4+CuSO_4\to Cu+Fe(SO_4)_3$

The reaction above is a single substitution reaction.

A single substitution reaction is whereby one metal $(Fe)$ displaces another $(Cu)$ from a solution of one of its salts$(CuSO_4)$

More over, $Fe$ is on top of the reactivity series hence displaces $Cu$ at its bottom of the series.

$Fe$ is thus more active hence cannot be displaced in the reaction by $Cu$