In the titration of KMnO4 and C2H2O, the oxalic acid is the analyte, and potassium permanganate is the titrant. The oxidizing and reducing agents are potassium permanganate and oxalic acid, respectively.
Because the permanganate ion in an acidic medium is a very potent oxidizing agent, the reaction between potassium permanganate and oxalic acid is conducted in an acidic medium.
By introducing weak H2SO4, the acidic condition is maintained. No other indicator is required to determine the endpoint, as KMnO4 acts as an self-indicator.
What is the endpoint potassium permanganate titration?
In redox titration such as potassium permanganate (KMnO4) with oxalic acid (C2H2O4), the solution of oxalic acid is in a conical flask and the solution of potassium permanganate is filled in the burette.
When we perform titration, on reaction with oxalic acid, permanganate solution discharged its violet color. The endpoint is indicated by the appearance of a pale pink color. Potassium permanganate acts as a self-indicator in these titration.
Why is the color of KMnO4 purple before the titration and after the endpoint it is pink?
The answer to this question is found in the experiment. During the titration, the Mn oxidation number is +7 before the reaction and after the reaction, it forms mostly +2. As a result of this transition, the color evolved to be pink which is why we see pink at the endpoint.
Why is the endpoint in permanganate titration not permanent?
The excess permanganate ion slowly reacts with the relatively large concentration of manganese (II) ions at the endpoint, this is the reason that the color of KMnO4 at the end point of titration may disappear after some time.
Why is the endpoint in the titration of KMnO4 and H2C2O4 pink?
The reaction between potassium permanganate and oxalic acid and H2C2O4 is a redox reaction in which MnO4- is reduced to Mn2+ while (C2O4)2- is oxidized to form CO2. The color of Mn2+ is very pale pink, and in low concentrations, it is almost completely colorless.
The pink color that you observe at the titration's end point is caused by the one additional drop of MnO4-, which does not decolorize because there isn't any further (C2O4)2- present to react with it.
The contents of the flask dilute the excessively purple droplet, making it appear pink. This deep purple color drop is diluted with the contents of the flask and therefore appears pink.
Why do we add dilute H2SO4 in the titration of KmNO4 with oxalic acid?
Because KMnO4 acts as an oxidizing agent only in acidic environments, to create an acidic environment, diluted sulphuric acid is introduced.
What is the color change of KMnO4 in the acidic, alkaline, and neutral medium in titration?
- Due to Mn (2+, it turns from purple to a faint permanent pink color in an acidic medium.
- The color of the MnO2 precipitates changes in neutral media, going from purple to reddish brown.
- Mn(VI)O4(2-), 1-electron turns from purple to green in strongly alkaline media.
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