Why hcl should not be used for potassium permanganate titrations?

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Redox titration is demonstrated by the titration of potassium permanganate (KMnO₄) against oxalic acid (C₂H₂O₄). The activity of the indicator close to the endpoint is akin to the other visual colour titrations used in oxidation-reduction (redox) titrations. Aim: This experiment evaluated the concentration, molarity, and strength (KMnO₄) solution by titrating it against a 0.1M oxalic acid reference solution (COOH-COOH). Theory: KMnO₄ is an oxidizing agent that operates more effectively in acidic than in alkaline environments. As a result, potassium permanganate is only utilized in an acidic medium for quantitative analysis. The following reaction in an acidic medium might be used to show its oxidizing activity – Reaction – MnO₄⁻ + 8H⁺ + 5e⁻ 🡪 Mn2+ + 4H₂O. In this titration using KMnO₄, we utilise sulphuric acid. Purple is the colour of the solution containing MnO₄⁻ ion. The solution containing Mn+2 ions, on the other hand, is colourless. When potassium permanganate combines with a reducing agent, it also functions as a self-indicator. Oxalic acid is used as a reducing agent in the experiment, and KMnO4 is placed in an acidic medium of H2SO4. As a result, no indication is required because potassium permanganate is a self-indicator. The following reactions can be used to titrate oxalic acid against potassium permanganate: Reduction half-reaction: 2KMnO4 + 3H2SO4 🡪 K2SO4 + 2MnSO4 + 3H2O + O2 Oxidation half-reaction: H2C2O4 🡪 2CO2 + H2O + CO Resultant: 2MnO4- + 5C2O42- +16H+ 🡪...