You titrated a 25.00 mL solution of .0350 M oxalic acid with a freshly prepared solution of KMnO4. If it took 37.55 mL of this solution, what was the molarity of KMnO4?
We need a stoichiometric equation that represents the oxidation of oxalic acid by permanganate........
You should be able to know how to get this reaction by the method of half-equations.......we will address this later...
We have a molar quantity of
Given the stoichiometry expressed above, we need
As to how to access the redox equation we set up the individual redox equations. Deep purple permanganate ion,
Charge and mass are balanced as required......
Meanwhile oxalic acid is oxidized to carbon dioxide.......
When you perform this reaction, the endpoint is signalled by the disappearance of the deep purple colour of the permanganate ion to give the ALMOST colourless