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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.
This hydrogen peroxide then releases hydrogen peroxide: [(HO) 3 B(OOH)] − + H 2 O ⇌ B(OH) − 4 + H 2 O 2. Several metal hydroperoxide complexes have been characterized by X-ray crystallography. Some form by the reaction of metal hydrides with oxygen gas: [17] L n M−H + O 2 → L n M−O−O−H (L n refers to other ligands bound to the ...
Together with its conjugate base superoxide, hydroperoxyl is an important reactive oxygen species.Unlike • O − 2, which has reducing properties, HO • 2 can act as an oxidant in a number of biologically important reactions, such as the abstraction of hydrogen atoms from tocopherol and polyunstaturated fatty acids in the lipid bilayer.
Hydrogen peroxide becomes more stable with higher peroxide content. 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 ...
Bleach activators react with hydrogen peroxide in aqueous solution to form peroxy acids. Peroxy acids are more active bleaches than hydrogen peroxide at lower temperatures (<60 °C) but are too unstable to be stored in their active form and hence must be generated in situ.
The peroxide group is marked in blue. R, R 1 and R 2 mark hydrocarbon moieties. The most common peroxide is hydrogen peroxide (H 2 O 2), colloquially known simply as "peroxide". It is marketed as solutions in water at various concentrations. Many organic peroxides are known as well. In addition to hydrogen peroxide, some other major classes of ...
Barium peroxide – unstable, spontaneously decomposes, compositions containing it should not be stored; Strontium peroxide; Lead tetroxide – versatile but toxic; Lead dioxide – used in friction-sensitive compositions, e.g. matches; Bismuth trioxide – used as a safe alternative to lead tetroxide in some compositions
All the hydrogen polyoxides are known or expected to autoionise when in liquid form, with the acidic hydrogen being solvated by other of the neutral polyoxide molecules. H 2 O n ⇌ H + + HO – n 2 H 2 O n ⇌ H 3 O + n + HO – n. The ions can also be formed by protonation or deprotonation of various neutral hydrogen polyoxide by suitably ...