MnO2 reacts with KOH to potassium permanganate in presence of KNO3 which acts as an oxidizing agent. The reaction is given as follows:
K2MnO4 is dark green in color implies that this is compound (A).
Potassium permanganate disproportionates in acidic solution to give an oxidized and reduced form of Mn ion
Compound (B) is KMnO4
Compound (B) is oxidizes KI solution which implies that it should itself undergo reduction, and as permanganate ion has +7 oxidation state of manganese it can no longer undergo oxidation and acts as a strong oxidation agent that oxidizes KI. Under alkaline medium:
Oxidized compound KIO3 is (C)
Under acidic conditions:
Compound (D) is I2, and orange brown color is obtained.
NOTE: the balancing of above two reactions is done with the help of oxidation number balancing in acidic and basic medium as mentioned in the question.
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