To balance the redox reaction between permanganate ion MnO4- and hydrogen peroxide H2O2 in an acidic solution, we need to follow these steps:1. Write down the half-reactions:MnO4- Mn^2+ reduction H2O2 O2 oxidation 2. Balance the atoms other than O and H in each half-reaction:MnO4- Mn^2+ already balanced 3. Balance the oxygen atoms by adding H2O molecules:MnO4- Mn^2+ + 4H2O4. Balance the hydrogen atoms by adding H+ ions:MnO4- + 8H+ Mn^2+ + 4H2O5. Balance the charge by adding electrons e- :MnO4- + 8H+ + 5e- Mn^2+ + 4H2O reduction half-reaction Now, balance the oxidation half-reaction:6. Balance the oxygen atoms by adding H2O molecules:H2O2 O2 + H2O7. Balance the hydrogen atoms by adding H+ ions:H2O2 + 2H+ O2 + 2H2O8. Balance the charge by adding electrons e- :H2O2 + 2H+ + 2e- O2 + 2H2O oxidation half-reaction 9. Balance the number of electrons in both half-reactions by multiplying each half-reaction by an appropriate factor:Reduction: MnO4- + 8H+ + 5e- Mn^2+ + 4H2OOxidation: 2 H2O2 + 2H+ + 2e- O2 + 2H2O 10. Add the half-reactions together and simplify:MnO4- + 8H+ + 5e- + 2H2O2 + 4H+ + 4e- Mn^2+ + 4H2O + 2O2 + 4H2OSimplified:MnO4- + 2H2O2 + 6H+ Mn^2+ + 2O2 + 4H2OSo, the balanced redox reaction for the reaction between permanganate ion MnO4- and hydrogen peroxide H2O2 in an acidic solution is:MnO4- + 2H2O2 + 6H+ Mn^2+ + 2O2 + 4H2O