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How can impure copper be purified using an electrolytic cell?
PrakritAllapur
When a strip of impure metallic copper is used as the anode in the electrolysis of an aqueous preparation of copper(II) sulfate, copper is oxidized. The oxidation of copper is more facile than the oxidation of water (see the standard oxidation potentials below) so metallic copper dissolves into solution as copper(II) ions, leaving behind many of the impurities (less active metals):
Cu(s) Cu2+(aq) + 2 e- (anode)
E°ox(Cu) = -0.34 V vs. E°ox(H2O) = -1.23 V
The copper(II) ions formed at the anode migrate to the cathode where they are more easily reduced than water and metallic copper "plates" on the cathode where it can be collected:
2 e- + Cu2+(aq) Cu(s) (cathode)
E°red(Cu2+) = +0.34 V vs. E°red(H2O) = -0.80 V
We had to pass sufficient current between the electrodes to cause the otherwise non-spontaneous reaction to occur! By carefully regulating the electrical potential, the metallic impurities that are active enough to be oxidized with copper at the anode are not reduced at the cathode and copper is selectively deposited
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