Hydrogenperoksid

Hydrogenperoksid, chemical formula H2O2, is a pale blue liquid in its concentrated form and a colorless solution when diluted. It is a widely used oxidizing agent found in household antiseptics, bleaching agents, and many industrial processes. Its solutions are miscible with water and vary in concentration from small amounts in first aid products to concentrated solutions used in industry. Hydrogen peroxide was first prepared by Louis Jacques Thénard in 1818.

Chemically, hydrogen peroxide decomposes slowly at room temperature into water and oxygen: 2 H2O2 → 2 H2O + O2. The reaction is exothermic and can be accelerated by heat, light, trace metals, or catalytic surfaces. Because of its strong oxidizing power, concentrated hydrogen peroxide can pose hazards, including caustic burns and rapid decomposition that may generate heat and oxygen gas. It is typically stored in dark, cool conditions in containers designed to limit contact with catalysts and organics. Stabilizers or inhibitors are sometimes added to commercial solutions to improve shelf life.

Industrial production is dominated by the anthraquinone process, in which a substituted anthraquinone is cyclically reduced and oxidized with air to generate hydrogen peroxide in solution, which is then separated and concentrated. This method allows scalable production and the generation of hydrogen peroxide at various concentrations for different applications.

Applications of hydrogen peroxide are broad. It is used for disinfection and sterilization, whitening and bleaching of paper, textiles, and hair, and as a chemical oxidant in various syntheses. It has also been employed as a rocket propellant oxidizer in certain historic and specialized applications. Environmental and safety considerations include its strong oxidizing nature and potential toxicity to aquatic life at high concentrations.

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