[robertss]

I know you can figure out how "strong" an oxidizing agent is by finding its Standard Reduction Potential (V).
I know for example, F2 is a better oxidizing agent than Co3+ because it has a more positive E value.
But how would you compare, lets say, "AgCl" or PbCl2 and their strength as oxidizing agents to F2?

Would you add the standard reduction potentials of the half reactions?
Could someone show me how this is done with AgCl vs. Cu2+, for example?

Thanks you

[Schrödinger]

I think that would depend on the reactions, because it is possible that either of the ions in AgCl(say) remains a spectator ion.