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How can I manually enter a lead-acid battery cell with the school laboratory?
These include aqueous sulfuric acid, lead sheet and lead dioxide powder. How do I create a simple implementation of cell, only to test voltage?
The sulfuric acid should be pretty concentrated. Auto batteries use about 35% H2SO4 by mass so that the ionization of the acid does not go to completion. You need HSO4 1+ ions for an effective cell.
You should probably do this experiment in a sturdy glass container. Pb sheet will be the anode, and PbO2 will be the cathode. If your PbO2 is loose powder, you will need to contain it somehow. I suggest packing the power stiffly in a test tube around a graphite core (you can obtain the graphite from thick pencil refills or an old lantern battery).
Now that you have an anode and a cathode, you can assemble the cell. Add your concentrated acid to the glass container (keep it well below the edge of the container). Attach conducting wire (copper wire is good, if you have it) to a piece of lead sheet, and sink into the solution. Be careful not to let the wire touch the solution! Attach another wire to the graphite sticking out of your test tube. Lower the test tube into solution until the Pb02/graphite is soaked, being careful not to let the wire touch the solution or to let the tube tip over. Now, connect each end of the wire to a voltmeter. There’s your voltage. If you don’t get a reading, try switching the wires.
Notes of caution:
- If you see bubbles, it is probably hydrogen gas. Take care to ventilate your experiment to prevent an explosive build-up.
- The acid is very corrosive. Be careful in handling and use eye protection before you even enter the lab.
- Lead is toxic. Don’t lick your fingers. Also do the world a favor and find some safe way to dispose of the PbSO4 lead solution you are generating. Dissolved lead is far more toxic than the solid metal.