0 m so42 150 m no3 010 m pb2 m pbno320050

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Unformatted text preview: for 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 Part I. 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.

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