In: Chemistry
Balance redox reaction in basic solution: Fe(OH)2(s) + MnO4-(aq) -> MnO2 (s) + Fe(OH)3
Fe in Fe(OH)2 has oxidation state of +2
Fe in Fe(OH)3 has oxidation state of +3
So, Fe in Fe(OH)2 is oxidised to Fe(OH)3
Mn in MnO4- has oxidation state of +7
Mn in MnO2 has oxidation state of +4
So, Mn in MnO4- is reduced to MnO2
Reduction half cell:
1 MnO4- + 3e- --> 1 MnO2
Oxidation half cell:
1 Fe(OH)2 --> 1 Fe(OH)3 + 1e-
Balance number of electrons to be same in both half reactions
Reduction half cell:
1 MnO4- + 3e- --> 1 MnO2
Oxidation half cell:
3 Fe(OH)2 --> 3 Fe(OH)3 + 3e-
Lets combine both the reactions.
1 MnO4- + 3 Fe(OH)2 --> 1 MnO2 + 3 Fe(OH)3
Balance Oxygen by adding water
1 MnO4- + 3 Fe(OH)2 + 1 H2O --> 1 MnO2 + 3 Fe(OH)3
Balance Hydrogen by adding H+
1 MnO4- + 3 Fe(OH)2 + 1 H2O + 1 H+ --> 1 MnO2 + 3 Fe(OH)3
Add equal number of OH- on both sides as the number of H+
1 MnO4- + 3 Fe(OH)2 + 1 H2O + 1 H+ + 1 OH- --> 1 MnO2 + 3 Fe(OH)3 + 1 OH-
Combine H+ and OH- to form water
1 MnO4- + 3 Fe(OH)2 + 1 H2O + 1 H2O --> 1 MnO2 + 3 Fe(OH)3 + 1 OH-
Remove common H2O from both sides
Balanced Eqn is
1 MnO4- + 3 Fe(OH)2 + 2 H2O --> 1 MnO2 + 3 Fe(OH)3 + 1 OH-
This is balanced chemical equation in basic medium
MnO4- + 3 Fe(OH)2 + 2 H2O --> MnO2 + 3 Fe(OH)3 + OH-