How do we represent the oxidation of ethanol to acetic acid, accompanied by the reduction of potassium permanganate to manganese(IV) oxide?
Well let us try it..........
Permanganate is reduced to
Ethanol is oxidized to
We add the individual redox reactions in such a way as to eliminate the electrons, i.e.
But basic conditions were specified, and thus we add
To give finally.......
The which I think is balanced with respect to mass and charge; as indeed it must be if we purport to represent chemical reality. What would see in the reaction? The intense, deep purple colour of permanganate ion would dissipate to give a brown precipitate of
Note that I am still not happy with this solution. Manganate ion, i.e.
I will let you do the adding of this to the oxidation equation.......