# What is the difference between balancing a redox reaction in acidic solution vs basic solution?

I'm asked to balance the potassium permanganate and hydrogen peroxide reaction. I misread the problem and thought that the reaction was in acidic solution. This is the result that I've got:

$$\ce{2MnO4 + 5H2O2 + 6H+ -> 2Mn^2+ +5O2 +8H2O}$$ What do I have to change to balance the equation in a basic solution?.

• The best approach is not to think in terms of changing this equation, but to just start over from scratch. Apr 30, 2017 at 17:54

$$\ce{2MnO4 + 5H2O2 + 6H+ + \color{blue}{6OH-} -> 2Mn^2+ +5O2 +8H2O + \color{blue}{6OH-}}$$
$\ce{H+}$ and $\ce{OH-}$ ions can be collectively re-written as $\ce{H2O}$, so we have:
$$\ce{2MnO4 + 5H2O2 + \color{blue}{6H2O} -> 2Mn^2+ +5O2 +8H2O + 6OH-}$$
$$\ce{2MnO4 + 5H2O2 -> 2Mn^2+ +5O2 +2H2O + 6OH-}$$