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?
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