Problem: Balance the following reaction:MnO4-(aq) + CH3OH(aq) → Mn2+(aq) + HCO2H(aq) (acidic solution)

We are being asked to balance the given oxidation-reduction reaction. The reaction is under acidic conditions. When balancing redox reactions under basic conditions, we will follow the following steps.

Step 1: Separate the whole reaction into two half-reactions

Step 2: Balance the non-hydrogen and non-oxygen elements first

Step 3: Balance oxygen by adding H₂O to the side that needs oxygen (1 O: 1 H₂O)

Step 4: Balance hydrogen by adding H⁺ to the side that needs hydrogen (1 H: 1 H⁺)

Step 5: Balance the charges: add electrons to the more positive side (or less negative side)

Step 6: Balance electrons on the two half-reactions

Step 7: Get the overall reaction by adding the two reactions.

Balancethe redox reaction under acidic conditions:

MnO₄^-_(aq) + CH₃OH_(aq) → Mn²⁺_(aq) + HCO₂H_(aq)

*Before balancing the redox reaction:

•ignore H⁺, OH^-, and H₂O in the starting reaction