Although many laboratory investigations and demonstrations use United States pennies (1-5), relatively little chemistry has been done with the penny's big brother, the "nickel". A United States 5-cent coin is made of an alloy that is 25% nickel and 75% copper (6). In this experiment, students isolate copper from a 5-cent coin using electrolysis (an example of the process of electrorefining). The isolation of pure copper metal from a coin that, at first glance, appears to be devoid of copper is a transformation that is both entertaining and highly educational for students ( Figure 1).
Electrolysis in a Chloride SolutionRefining of metals through electrolysis can be performed either through a process of selective oxidation or selective reduction (7). In this experiment, pure copper is obtained through a process of selective reduction. The 5-cent coin is used as the anode and a graphite rod is used as the cathode. 6 M HCl is used as the electrolyte. HCl is chosen as the electrolyte for two reasons: the acidity promotes the solubility of the transition metal ions produced during electrolysis, and the chloride ions form coordination complexes that also enhance the solubility of the transition metal ions. A schematic diagram of the experimental setup is shown in Figure 2.When electrolyzed in typical aqueous solutions, the metals that make up the 5-cent coin are oxidized according to the half-reactions:However, when a significant concentration of chloride ion is present in the electrolytic bath, the following oxidation halfreaction for copper is favored (8,9):CuCl is almost insoluble in water, but in a bath of 6 M HCl, the CuCl will react with additional Cl − ions to form soluble complexes such as CuCl 2 − and CuCl 3 2− (9). This solubility allows the copper ions to migrate through solution to eventually become reduced at the cathode.
Experimental ObservationsDuring the experiment, the 5-cent coin is gradually dissolved, resulting in an intensely green-colored electrolyte bath. The green color of the bath results from aqueous Ni 2+ ions (which may react with excess chloride ions to form complex ions such as NiCl 4 2− ). The copper(I) chloride complexes are nearly colorless, but may slowly (over a period of hours) be air oxidized to form green copper(II) chloride complexes (10).In a bath containing aqueous H + ions, Cu + complex ions, and Ni 2+ ions, the important reduction potentials are:CuCl + e − → Cu(s) + Cl − E Њ = +0.14 V 2H + + 2e − → H 2 (g) E Њ = +0.00 V Ni 2+ + 2e − → Ni(s) E Њ = ᎑0.25 V During the first few minutes of this electrolysis experiment, only hydrogen gas is formed at the cathode, but soon, as the