ATAR Notes: Forum
VCE Stuff => VCE Science => VCE Mathematics/Science/Technology => VCE Subjects + Help => VCE Chemistry => Topic started by: #1procrastinator on September 13, 2012, 06:55:42 pm
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Why does the solution need to have the ions of the metal you use for plating? Are these ions used in plating whatever you're plating?
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You need to have an oxidant and a reductant, and those ions are reduced on the surface of the electrode reductant (the electrode) to form the metal which you're plating.
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Why can't you just use water and get the ions from the electrode?
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^, Wouldn't it depend on the context of the question?
Like, Water could interfere with the reaction and itself could be the stronger oxidant/reductant and hence, itself would be reduced/oxidised.
.... Correct me if I'm wrong.
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^ I'm just trying to gain a conceptual understanding at the moment. IF water interferes with itself, then shouldn't it do so even with the ions (hence the molten state stuff)?