Oxidation With Permanganate

Oxidation with permanganate refers to a chemical reaction in which permanganate ion (MnO4-) acts as an oxidizing agent and oxidizes another compound or molecule. The oxidation reaction involves the transfer of electrons from the compound being oxidized to the permanganate ion, causing it to be reduced to a different form.

The process of oxidation with permanganate is often used in analytical chemistry as a qualitative test to identify reducing agents or compounds that can be oxidized by permanganate. It is also used in organic chemistry for the synthesis of certain compounds.

In acidic conditions, permanganate ion is reduced to manganese(II) ion (Mn2+) according to the following half-reaction:

MnO4- + 8H+ + 5e- → Mn2+ + 4H2O

Meanwhile, the substance being oxidized undergoes reduction, releasing electrons in the process:

X → Xn+ + ne-

Overall, the chemical equation for the oxidation of X by permanganate ion in acidic solution can be written as:

MnO4- + 8H+ + 5e- → Mn2+ + 4H2O

X → Xn+ + ne-

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MnO4- + 8H+ + X → Mn2+ + Xn+ + 4H2O

The number of electrons transferred in the reduction half-reaction determines the stoichiometry of the reaction, which allows for the determination of the amount of X present in the sample being analyzed.

The use of permanganate as an oxidizing agent is limited to acidic conditions, as at high pH values, it disproportionates to form manganese dioxide and oxygen gas, thereby reducing its effectiveness as an oxidizing agent.