hypochloriti

Hypochlorite refers to the hypochlorite ion, ClO−, and to compounds that contain it. It is the conjugate base of hypochous acid (HClO). In aqueous solution, hypochlorite acts as a powerful oxidizing agent and is widely used for disinfection and bleaching. The term is used in several languages, and hypochloriti or hypochlorito may appear as the plural or corresponding term in some contexts.

Common hypochlorites include sodium hypochlorite (NaOCl), calcium hypochlorite (Ca(OCl)2), and potassium hypochlorite (KOCl). Sodium hypochlorite is most familiar as a dilute household solution (active chlorine typically about 3–6%). Calcium hypochlorite is sold as a solid with higher available chlorine content, used for water treatment and sanitation. These compounds differ in stability and handling: sodium hypochlorite solutions are easier to dilute and store, while solid calcium hypochlorite is more energy-dense but more reactive.

Production typically involves the reaction of chlorine with alkali or alkaline materials. A common route is Cl2 + 2 NaOH → NaOCl + NaCl + H2O, producing sodium hypochlorite in solution. Calcium hypochlorite is produced by reacting chlorine with calcium hydroxide. The resulting products are strong oxidizers and can release chlorine gas if acidified or heated.

Uses of hypochlorites include disinfection of drinking water, sanitation of surfaces and equipment, and bleaching in the pulp and paper and textile industries. They are also employed in food processing and medical settings for surface sterilization. Safety considerations include their corrosive and reactive nature; they should be kept away from acids and organic materials, stored cool and protected from heat, and handled with appropriate protective equipment. Environmental considerations involve degradation to chloride and, under certain conditions, chlorate byproducts.