Redox titrations with potassium permanganate — practice questions
5 questions in the bank on this idea. Below are 5 of them, exactly as they appear in a test.
Why is potassium permanganate described as a self-indicator in many redox titrations?
- A. It produces a fluorescent precipitate at equivalence
- B. It becomes colourless before any reaction begins
- C. It releases a separate acid-base indicator
- D. A slight excess gives a persistent colour
Which acid is preferred for acidifying a potassium permanganate redox titration?
- A. Dilute sulphuric acid
- B. Concentrated hydrochloric acid
- C. Concentrated nitric acid
- D. Aqueous acetic acid as the universal choice
In strongly acidic solution, permanganate ion is reduced mainly to which manganese species?
- A. MnO2
- B. Mn2+
- C. MnO4^2−
- D. Mn metal
An oxalate-permanganate titration is very slow at room temperature but becomes faster after gentle warming. What explains this?
- A. Oxalate cannot exist below its boiling point
- B. Warming converts permanganate into an acid-base indicator
- C. Warming helps overcome the reaction's activation barrier
- D. Heating prevents all manganese ions from forming
A permanganate titration is continued until the solution becomes a deep purple rather than a faint permanent pink. What is the most likely consequence?
- A. The analyte amount has increased during titration
- B. The endpoint has not yet been reached
- C. The titrant concentration has become exactly zero
- D. Endpoint overshot; titre too high
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