Oxidation states of manganese and pH

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SUMMARY

The discussion focuses on the stability of manganese oxidation states in relation to pH levels. It is established that manganese (Mn) acts as a stronger oxidizing agent in acidic conditions compared to basic ones. This leads to the conclusion that higher oxidation states of manganese are more stable in alkaline environments. Additionally, the formation of a brown precipitate in permanganate solutions raises questions about the decomposition reaction and its products.

PREREQUISITES
  • Understanding of manganese oxidation states
  • Knowledge of acid-base chemistry
  • Familiarity with redox reactions
  • Basic principles of chemical equilibrium
NEXT STEPS
  • Research the stability of manganese oxidation states in various pH conditions
  • Study the decomposition reactions of permanganate ions
  • Explore the role of pH in redox reactions
  • Investigate the formation and properties of manganese precipitates
USEFUL FOR

Chemistry students, researchers in inorganic chemistry, and professionals studying redox reactions and manganese chemistry.

Moogie
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Hi

I am interested in the change in the stability of the oxidation states of manganese with pH

Mn is a stronger oxidising agent in acid than in base which would lead you to believe that the higher oxidation states of Mn are more stable in alkaline conditions.

Does anyone have a reason why? I couldn't find one

Thanks
 
Physics news on Phys.org
There is a brown precipitate forming in solutions of permanganate. Have you tried to write reaction equation for the decomposition reaction? What are products of the decomposition?
 
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