Problem: A 1L solution containing 0.110 M NiCl 2(aq) and 0.200 M CuBr2(aq) is subjected to electrolysis.How much time would it take to selectively plate out one of the cations at a current of 5.0 A?

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We’re being asked to calculate for the time it would take to selectively plate out one of the cations in the given solution.

The solution is made up of 0.110 M NiCl2(aq) and 0.200 M CuBr2(aq) and subjected to electrolysis. Both will break up in the solution:

NiCl2(aq) → Ni2+(aq) + 2 Cl-(aq)

CuBr2(aq) → Cu2+(aq)+ 2 Br-(aq) 


Let’s first determine which cation (positively charged ion) will be plated out from the solution first. The one with the higher reduction potential will be plated out first.

*the standard reduction potential table (E°cell values) can be found in books or on the internet

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Problem Details

A 1L solution containing 0.110 M NiCl 2(aq) and 0.200 M CuBr2(aq) is subjected to electrolysis.

How much time would it take to selectively plate out one of the cations at a current of 5.0 A?


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