I am quite confusing about the concept of electroplating of silver. As what I know, the silver anode gives out Ag+ while the Ag+ in the silver nitrate solution deposits on the cathode (e.g. a spoon). However, why the Ag(s) on the silver anode is preferentially discharged instead of the OH- in silver nitrate solution? Here are the electrode potentials: O2(g) + 2 H2O + 4 e− <--> 4 OH−(aq) +0.4V Ag+ + e− <--> Ag(s) +0.8V O2(g) + 4 H+ + 4 e− <--> 2 H2O +1.23V As the process is carried out in alkaline condition, I suppose only the first two equations are involved. From the potential values, the OH- should be preferentially discharged rather than the Ag(s), but the actual situation is the opposite. I am not sure if I have misunderstood anything (e.g. the third equation is involved instead).