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Hydrogen peroxide is a chemical compound with the formula H 2 O 2.In its pure form, it is a very pale blue [5] liquid that is slightly more viscous than water.It is used as an oxidizer, bleaching agent, and antiseptic, usually as a dilute solution (3%–6% by weight) in water for consumer use and in higher concentrations for industrial use.
For example, the loss of blue color in leuco-methylene blue is selective for hydrogen peroxide. [21] Quantitative analysis of hydroperoxides can be performed using potentiometric titration with lithium aluminium hydride. [22] Another way to evaluate the content of peracids and peroxides is the volumetric titration with alkoxides such as sodium ...
Many industrial peroxides are produced using hydrogen peroxide. Reactions with aldehydes and ketones yield a series of compounds depending on conditions. Specific reactions include addition of hydrogen peroxide across the C=O double bond: R 2 C=O + H 2 O 2 → R 2 C(OH)OOH. In some cases, these hydroperoxides convert to give cyclic diperoxides:
For example, 98% hydrogen peroxide is more stable than 70% hydrogen peroxide. Water acts as a contaminant, and the higher the water concentration the less stable the peroxide is. The storability of peroxide is dependent on the surface-to-volume ratio of the materials the fluid is in contact with.
A closely related mixture, sometimes called "base piranha", is a 5:1:1 mixture of water, ammonia solution (NH 4 OH, or NH 3 (aq)), and 30% hydrogen peroxide. [2] [3] As hydrogen peroxide is less stable at high pH than under acidic conditions, NH 4 OH (pH c. 11.6) also accelerates its decomposition.
In chemistry, peroxides are a group of compounds with the structure R−O−O−R, where the R's represent a radical (a portion of a complete molecule; not necessarily a free radical [1]) and O's are single oxygen atoms. [2] [3] Oxygen atoms are joined to each other and to adjacent elements through single covalent bonds, denoted by dashes or lines.
In chemistry, the oxygen reduction reaction refers to the reduction half reaction whereby O 2 is reduced to water or hydrogen peroxide. In fuel cells, the reduction to water is preferred because the current is higher. The oxygen reduction reaction is well demonstrated and highly efficient in nature. [1] [2]
The Dakin oxidation can occur in mild acidic conditions as well, with a mechanism analogous to the base-catalyzed mechanism. In methanol, hydrogen peroxide, and catalytic sulfuric acid, the carbonyl oxygen is protonated (14), after which hydrogen peroxide adds as a nucleophile to the carbonyl carbon, forming a tetrahedral intermediate (15).