1. The problem statement, all variables and given/known data A redox titration is carried out by adding Purple KMnO4 solution from a burette to a solution of H2O2 in a flask. Which of the following would occur in the flask before the equivalence point is reached? The answer is: The solution is colorless and O2 is formed. The other options were that the solution would remain purple and O2 gas would form, that the solution would remain purple and H2 gas would form, and the solution would be colourless and O2 gas would form. 2. Relevant equations So my table says: H2O2 + 2H+ + 2e- <=> 2 H20 has a reduction potential of +1.78 And Mn04 + 8H= + 5e- <=> Mn2+ + 4H20 has a reduction potential of +1.51 3. The attempt at a solution Shouldn't H2O2 be the oxidizing agent, forming H2O?