Reaction of Manganese and hydrogen peroxide

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Discussion Overview

The discussion revolves around the reaction of manganese ions with hydrogen peroxide in a laboratory setting, focusing on the chemical equilibria involved, the formation of precipitates, and the potential oxidation states of manganese. The scope includes experimental observations and chemical reasoning related to redox reactions and precipitate formation.

Discussion Character

  • Exploratory, Technical explanation, Experimental/applied

Main Points Raised

  • One participant describes the equilibria of Mn2+ ions in water and the effect of NaOH on this equilibria, leading to the precipitation of Mn(OH)2.
  • The same participant notes the addition of hydrogen peroxide results in gas release and a brown precipitate, speculating that the peroxide oxidizes Mn2+ ions.
  • Another participant challenges the ease of forming Mn2O3, suggesting it may not be straightforward.
  • A different participant proposes that MnO2 is the precipitate formed and references the redox reaction of hydrogen peroxide under basic conditions.
  • One participant expresses agreement with the idea of MnO2 being the product.

Areas of Agreement / Disagreement

Participants express differing views on the specific manganese oxide formed, with some proposing MnO2 and others questioning the feasibility of Mn2O3. The discussion does not reach a consensus on the identity of the precipitate or the balancing of the reaction.

Contextual Notes

The discussion includes assumptions about the oxidation states of manganese and the conditions under which the reactions occur, which are not fully resolved. The exact nature of the precipitate and the balancing of the overall reaction remain unclear.

Moogie
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Hi

In a recent lab I reacted Mn2+ ions with NaOH. The Mn 2+ ions exist in this equilibria

[Mn(H20)6]2+ + H20 <=>
[Mn(H20)5OH]+ + H30+

Addition of NaOH ions shift this equilibria to the left (by removing protons) until Mn(OH)2 is precipitated

Hydrogen peroxide is then added and some gas is released and a brown precipiate formed. I presume the peroxide is oxidising the Mn2+ ions but I don't know what the precipitate is or how to balance the reaction. Some possibilities are Mn02 and Mn2O3 which are manganese oxides in a higer oxidation state.

thanks
 
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Mn2O3 is not that easy to make.
 
I went for MnO2. I also used the redox reaction for hydrogen peroxide under basic conditions
 
Sounds reasonable.
 
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