In the electrolysis of dilute sulphuric acid, I'm given these two half-equations:
anode: 4OH-(aq) -> 2H2O(l) + O2(g) + 4e-
cathode: 4H+(aq) + 4e- -> 2H2(g)
Why does the concentration of hydrogen ions increase?
Isn't the concentration of hydrogen ions decreasing here, rather than increasing as it is being discharged at the cathode?
N.B: (This question originates from a past AQA GCSE Question: see question 2 part (d) here.)