Electrolysis of aq CuCl2 with Ag electrode

I have a question on electrolysis:

In the electrolysis of aq Copper (II) Chloride using silver electrodes, what are the products?

Cathode : Copper or silver are deposited here? cos both are in the solution

anode : silver electrode decrease in size... with silver deposits?

Am I correct?

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You need to know the voltage applied and you need to know what is the cathode and what is the anode.

Mentor
using silver electrodes

you need to know what is the cathode and what is the anode.

Seems like that's a given.

Basically the question can be split in two:

What is the reaction on anode? What are possibilities?

What is the easiest to reduce substance present in the solution, one that will be reduced first?

And don't forget about chlorides presence. Concentration is not given, but it may be not that important, perhaps it will be possible to estimate what is happening without knowing exact numbers.

Homework Helper
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Seems like that's a given.

Basically the question can be split in two:

What is the reaction on anode? What are possibilities?

What is the easiest to reduce substance present in the solution, one that will be reduced first?

And don't forget about chlorides presence. Concentration is not given, but it may be not that important, perhaps it will be possible to estimate what is happening without knowing exact numbers.

I misunderstood. TWO ELECTRODES, both Silver.

So if electrolysis will occur, the Cu+2 will become reduced to Cu metal at one particular electrode, and Ag+ will form and go into solution at the other electrode.

Mentor
So if electrolysis will occur, the Cu+2 will become reduced to Cu metal at one particular electrode, and Ag+ will form and go into solution at the other electrode.

Not necessarily. But let's allow OP to answer the question this time.

Homework Helper
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Cu+2 could be reduced to Cu+1, depending on voltage and conditions of solution; not sure if this is reasonable for electrolysis. Probably is.

it's confusing at the cathode - cos both Ag+ (from the anode) and Cu2+ (from the electrolyte ) are present.
Its more of a simple set up without going into too much details. Its for O level type of question.
Concentration - aqueous solution.

Homework Helper
Gold Member
it's confusing at the cathode - cos both Ag+ (from the anode) and Cu2+ (from the electrolyte ) are present.
Its more of a simple set up without going into too much details. Its for O level type of question.
Concentration - aqueous solution.

Good attention to detail, there. Yes, if the anode is producing Ag+, then the cathode could be depositing Ag and either plating Cu0 or making Cu+1. My wits stop there.

Mentor
it's confusing at the cathode - cos both Ag+ (from the anode) and Cu2+ (from the electrolyte ) are present.
Its more of a simple set up without going into too much details. Its for O level type of question.
Concentration - aqueous solution.

Honestly - I have no idea what the intended answer is. Remember that silver concentration is limited by the silver chloride solubility in the presence of chlorides from copper chloride. That means it all depends on the concentration of CuCl2. For low concentrations silver dissolves and deposits, Cu2+ is just a spectator. For higher concentrations - copper deposits till its concentration is so low silver starts to deposit. "Aqueous solution" doesn't tell anything about concentration, it can be anything - saturated copper chloride solution is close to 2M, diluting it to 10-5M is five minutes work. Limiting concentration (one that changes the experiment outcome) lies in between.