Electrolysis is used to obtain pure copper, because when it is obtained by reduction from its ore its not pure enough for use in electric conductors.
The electrolyte is copper II sulfate solution. The cathode starts as a thin peice of pure ion and more pure copper adds to it during the reaction. The anode is a big lump of pure copper which will dissolve.
The electrical supply pulls copper atoms off the anodle, causing them to go back into the solution as Copper 2+ ions. The offering electrons at the cathode near to the Copper 2+ ions turn them back into copper atoms. The impurities are dropped at the anode as a sludge, whilst the pure copper atoms bond to the cathode.
Pure copper is deposited on the negative cathode. Copper ions are reduced to copper atoms by gaining electrons. Cu2+ + 2e- = Cu(s)
Copper dissolves from the impure positive anode. Copper atoms are oxidised into copper ions by losing electrons. Cu(s) = Cu2+(aq) + 2e-
The mass of the anode and cathode will change - movement of copper ions. To measure, weigh anode + cathode before. Put in copper sulfate solution, connect power pack for 5 mins. Remove, dry, weigh anode+cathode. Anode should be less, cathode more.
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