write the balanced equation for the reaction please and indicate the oxidation state of the(Mn) in the product

Question

Permanganate ion, ( MnO 4) - oxidizes SULFITE ions to SULFATE ion. The manganese (Mn) product depends on the pH of the reaction mixture. The mole ratio of oxidizing to reducing agent is 2 to 5 at pH 1 amd jas a ratop pf 2 to 1 at pH 13. For each of these cases please explain and write the balanced equation for that rxn. and indicate the oxidation states.


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Answer 1

There is only one equation for the reaction. The net ionic equation for this is:

2 (MnO4)- + 5 (SO3)-2 + 6 H+ = 2 Mn+2 + 5 (SO4)-2 + 3 H2O

which is the electron balanced sum of the two half reactions:

(MnO4)- + 8 H+ + 5 e- = Mn+2 + 4 H2O and

(SO3)-2 + H2O = (SO4)-2 + 2 H+ + 2 e-

an increase in H+ (decrease in pH) drives the reaction to the right while an increase in pH drives it to the left.

Mn has an oxidation state of +7 on the left and +2 on the right.
S has a +4 on the left and a +6 on the right.