Potassium Permanganate Reduction in Aqueous Buffer

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SUMMARY

The discussion centers on the reduction of potassium permanganate in an aqueous buffer containing 1M ammonia and ammonium, treated with 1M sodium hypochlorite. The permanganate ion is reduced to insoluble manganese dioxide while the hypochlorite ion is oxidized to perchlorate ion. A key point of contention is the pH of the solution; despite the presence of a buffer, the solution is considered acidic, raising questions about the accuracy of the notes provided. The confusion stems from the properties of the buffer and the behavior of the hypochlorite ion as a weak Brønsted-Lowry base.

PREREQUISITES
  • Understanding of redox reactions and oxidation states
  • Knowledge of buffer solutions and their pH effects
  • Familiarity with Brønsted-Lowry acid-base theory
  • Basic chemistry of potassium permanganate and sodium hypochlorite
NEXT STEPS
  • Research the properties of ammonia and ammonium buffers
  • Study the redox reactions involving potassium permanganate and sodium hypochlorite
  • Examine the pH behavior of weak bases in buffered solutions
  • Learn about the formation and properties of manganese dioxide in redox reactions
USEFUL FOR

Chemistry students, researchers in analytical chemistry, and professionals involved in redox chemistry and buffer systems will benefit from this discussion.

Kruz87
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Hello everybody,
I'm told that potassium permanganate is dissolved in an aqueous buffer of ammonia and ammonium at equal concentrations (1M), and treated with 1M sodium hypochlorite, the permanganate ion is reduced to insoluble manganese dioxide as the hypochlorite ion is oxiddized to perchlorate ion.

I have the notes to the solution of the problem, but I noticed that he considered the solution to be acidic?

Why?
The buffer should have no affect on pH and OCl^- is a weak bronstend lowry base. So why wouldn't the solution be basic?
 
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I don't know why. Could it be there's a mistake in the notes?
 

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