1. The problem statement, all variables and given/known data Fe(NH4)2(SO4)2*6H2O is mixed with H2SO4 and then titrated with KMnO4 until the equivalence point is reached. The question I am confused with is: What might have been the product(s) in the original solution if it had remained neutral? (if the solution was not acidified with H2SO4) How could you determine this? 2. Relevant equations Net Ionic Equation: 8H+ + MnO4- + 5Fe2+ => Mn2+ + 4H2O + 5Fe3+ 3. The attempt at a solution From the wikipedia page on this, it says that potassium permanganate degrades into MnO2 when reacted in a neutral equation. I would think that the redox reaction would still occur between the Fe2+ solution and the KMnO4, but it wouldn't reach the equivalence point since there is no acid...so it wouldn't change color?