hydrogenperoxide

Hydrogen peroxide is a chemical compound with the formula H2O2. It is a colorless, slightly viscous liquid that is miscible with water. In solution, its odor is faintly sharp. The molecule contains a peroxide bond (an O–O single bond), making it a relatively weak, but powerful, oxidizing agent.

Chemically, hydrogen peroxide acts as an oxidizer in many reactions and decomposes to water and oxygen. The decomposition is catalyzed by heat, light, or catalysts such as manganese dioxide or iodide. In concentrated form, it can decompose rapidly, releasing oxygen gas; this property underpins both its uses and safety considerations. Stabilizers are often employed in commercial solutions to slow unwanted decomposition.

Industrially, hydrogen peroxide is mainly produced by the anthraquinone process and distributed in stabilized aqueous solutions. Concentrations vary: household products are typically around 3%, with higher concentrations used in laboratories and industry. Concentrated solutions, including higher-test peroxide used in some propulsion systems, are handled with strict safety controls.

Applications are diverse. It serves as a disinfectant and antiseptic, a bleaching agent for textiles and paper, and a cleaning agent in household and industrial contexts. In medicine, diluted solutions are used for surface disinfection and wound care, though concentration and use are important for safety. In industry, it is employed for bleaching, oxidative treatment of effluents, and as an oxidizer in chemical synthesis. Hydrogen peroxide naturally decomposes into water and oxygen, making it relatively environmentally benign when contained and managed properly.

History notes that hydrogen peroxide was first prepared by Louis Jacques Thénard in 1818 through the acidification of a peroxide salt, establishing its identity and potential uses.