To utilize oxidation-reduction reactions in the construction of a voltaic cell (chemical
to study its properties.
(2) 250-mL beakers
1M aluminum nitrate
1M lead nitrate
1M sodium chloride
Attach the lead electrode to the negative side of the voltmeter and the copper electrode
to the positive side.
Fill one beaker with Al(NO3)3 and the other with Pb(NO3)2.
Place the aluminum strip in the 1M Al(NO3)3 and the copper
electrode in the 1M Pb(NO3)2 solution.
Prepare a salt bridge by soaking a rolled paper towel in the 1M NaCl solution. Put one
end of the paper salt bridge in the 1M Al(NO3)3 solution and the
other end in the 1M Pb(NO3)2 solution.
Allow the cell to run for a few minutes. Examine the two metallic electrodes during this
period. The lead electrode should begin to dissolve and will become pitted. Aluminum metal
will begin to form at the surface of the alumninum metal electrode.
After you have allowed the cell to run for a few minutes, disconnect the wires from the
ata & Observations:
Write a balanced equation for the reaction taking place in this reaction.
Voltages listed in references for voltaic cells are given in terms of standard cell
potentials (voltages). What is meant by a standard cell? Was your initial voltaic cell a
As a standard voltaic cell runs, the voltage delivered by the cell drops. Why does this
Would you expect the voltage delivered by a voltaic cell to change with temperature? Why
or why not?