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An electrolytic process is the use of electrolysis industrially to refine metals or compounds at a high purity and low cost. Some examples are the Hall-Héroult process used for aluminium, or the production of hydrogen from water.

Crude Copper is not suitable to be used in to be used in electrical appliances because it has many impurities that reduce its conductivity. That is the reason why impure copper is obtained by the process of electrolysis where crude copper metal rod is used as anode and pure copper metal rod as cathode. As an electrolyte it is used an acidic solution of copper sulphate (CuSO₄).

When suitable voltage is applied to the electrode, it causes oxidation of copper metal at anode. As a result, Cu oxidize to Cu²⁺ in the solution which result to releasing electrons that are attracted by a cathode. Cu²⁺ ions in the solution gain electrons from the cathode and reduce to Cu which get deposited on cathode in its purest form. And this electrolytic reaction is reaction of copper purification.

Reaction on anode:\(Cu \to C{u^{2 + }} + 2{e^ - }\)

Reaction on cathode:\(C{u^{2 + }} + 2{e^ - } \to Cu(s)\)

Hence, the final answer is:

We use electrolysis to get pure form of copper.