【Basic Theory】At what pH or above does hydrogen peroxide exhibit reducibility?
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At what pH value or above does hydrogen peroxide exhibit reducing properties, and at what pH value or below does it exhibit oxidizing properties?
Hydrogen peroxide is reducitive at a pH of 7 or higher, and oxidizing at a pH lower than 7
This post was last edited by qugd on 2015-9-23 08:32. The oxidizing and reducing properties of hydrogen oxide are relative; judging them simply based on their acidity is neither objective nor accurate. It should be calculated using the redox potential under the appropriate conditions, and compared with the reactants in the reaction system. Additionally, hydrogen peroxide can undergo disproportionation reactions, acting as both an oxidizing agent and a reducing agent.
I see, it’s like that. I’ll take another look at the information. Thank you for your guidance, master
The redox approach is correct; to determine hydrogen peroxide, 1+15 sulfuric acid is used along with potassium permanganate for titration. This involves reduction in a strongly acidic environment. For the production of tetrabromobisphenol A, equal amounts of hydrogen peroxide and bromine are used, with hydrogen peroxide’s oxidizing property being utilized to convert hydrobromic acid into bromine – this is not oxidation under weakly acidic conditions.
Thank you for your guidance, master. To determine hydrogen peroxide, 1+15 sulfuric acid is used along with potassium permanganate for titration. Is the principle behind this the reducing property of hydrogen peroxide in a strongly acidic environment?
It indicates that potassium permanganate has strong oxidizing properties in acidic conditions