Galvanization refers to the process of covering steel or iron with zinc in order to protect the underlying metals from corrosion. Zinc, relatively, has far less of a corrosion resistance than iron and steel. Thus, zinc is consumed first as a sacrificial anode (negatively charged component). In the case of scratches through zinc, the underlying iron or steel will not rust because the iron or steel will be cathodically protected by its zinc covering. The process of galvanization, while straightforward, should only be carried out by an experienced professional.
- Zinc sulfate
- Deionized water
- Nonreactive bath
- Zinc strip
- Two-electrode system
- Voltage current source
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Instructions
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1
Dissolve 30 grams of zinc sulfate in a nonreactive bath (ie, ceramic) in 100 milliliters of water.
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2
Connect the metal to be galvanized to the anode (negative terminal) of a two-electrode system. Connect the cathode, or positive end, to a strip of zinc.
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3
Plug in the voltage current source, and connect to the bath. Immerse the two-electrode system in the bath, and run the current through the bath for 1 minute.