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May 30, 2024, 08:09:05 am
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Author Topic: Electroplating/electrolysis  (Read 1119 times)  Share 

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#1procrastinator

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Electroplating/electrolysis
« 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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charmanderp

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Re: Electroplating/electrolysis
« Reply #1 on: September 13, 2012, 06:57:15 pm »
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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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#1procrastinator

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Re: Electroplating/electrolysis
« Reply #2 on: September 14, 2012, 10:05:05 am »
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Why can't you just use water and get the ions from the electrode?
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Howzat

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Re: Electroplating/electrolysis
« Reply #3 on: September 14, 2012, 12:58:55 pm »
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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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#1procrastinator

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Re: Electroplating/electrolysis
« Reply #4 on: September 19, 2012, 08:08:54 pm »
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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)?
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