Question

# Mr. Ramu wants to electroplate his key chain with nickel to prevent rusting. For this electroplating: (i) Name the electrolyte (ii) Name the cathode (iii) Name the anode (iv) Give the reaction at the cathode (v) Give the reaction at the anode.

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Solution

## (i) Electrolyte - Aqueous solution of nickel sulphate (ii) Cathode - Cleaned key chain to be electroplated (iii) Anode - Block of nickel metal (iv) Reaction at cathode: From the electrolyte, the nickel ions gain electrons to form nickel atoms, that get deposited on the article (key chain) as a layer of nickel: ${\mathrm{Ni}}^{2+}+2{\mathrm{e}}^{-}\stackrel{}{\to }\mathrm{Ni}\phantom{\rule{0ex}{0ex}}\left(\mathrm{from}\mathrm{e}\mathrm{l}\mathrm{e}\mathrm{c}\mathrm{t}\mathrm{r}\mathrm{o}\mathrm{l}\mathrm{y}\mathrm{t}\mathrm{e}\right)\mathrm{N}\mathrm{i}\mathrm{c}\mathrm{k}\mathrm{e}\mathrm{l}\mathrm{d}\mathrm{e}\mathrm{p}\mathrm{o}\mathrm{s}\mathrm{i}\mathrm{t}\mathrm{e}\mathrm{d}\mathrm{o}\mathrm{n}\mathrm{a}\mathrm{r}\mathrm{t}\mathrm{i}\mathrm{c}\mathrm{l}\mathrm{e}$ (v) Reaction at anode: The nickel anode loses electrons to become nickel ions and goes into the electrolyte. $\mathrm{Ni}\stackrel{}{\to }{\mathrm{Ni}}^{2+}\left(\mathrm{into}\mathrm{electrolyte}\right)+2{\mathrm{e}}^{-}\phantom{\rule{0ex}{0ex}}\left(\mathrm{from}\mathrm{anode}\right)\mathrm{Nickel}\mathrm{ions}$

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