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the complete precipitation of PbSO4. Assemble and measure the voltage of the cell:
Cell #7 Pb(s) | PbSO4(s), NH4+ (3.0 M), SO42- (1.50 M), NO3- (0.10 M), Pb2+(? M) || Pb(NO3)2(0.050 M) | Pb(s) (This is experimentally very easy to do: fill one well of your spot plate with the diluted
lead nitrate solution, fill an adjacent one with a slurry of the contents of the test tube
containing the precipitated lead sulfate, connect them with salt bridge strings to a well
full of the sodium nitrate solution, attach two Pb electrodes to the wires from the meter,
and measure the cell voltage.)
Clean-up. Dispose of all the lead-containing solutions in the proper waste container
found in the fumehood. 16 DATA ANALYSIS
For every conventional galvanic cell diagram there is a corresponding (chemical) cell
reaction, as illustrated by the example in the Introduction section of this experiment.
According to the Nernst equation the conventional cell voltage of such a cell can be
written in general as
Ecell = (E°cathode - E°anode)- [0.0257 / n] ln Q
where E°cathode is the standard reductio...
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This note was uploaded on 04/09/2013 for the course CHE CHE 2C taught by Professor Nasiri during the Spring '07 term at UC Davis.
- Spring '07