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Unlike many other titrations no indicator is necessary to tell the experimenter when the endpoint of the reaction is. In this case, the experimenter knows when all the oxalate has been consumed because the excess of permanganate will show up as a pink color. Thus, the permanganate ion acts as an indicator itself. The reaction produces its own catalyst in the form of Mn2+ that promotes oxidation. The sulfuric acid added to the titration flask acts as a proton donor for the solution readily giving up protons. Since the oxalic acid is not a strong acid and does not dissociate well, but is still needed in the reaction to form carbon dioxide, the addition of a strong acid, sulfuric acid, supplies the protons needed for the reaction...
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