Hypochloritit

Hypochloritit refers to hypochlorite species and salts derived from hypochlorous acid (HOCl), collectively known as hypochlorites. The hypochlorite anion is ClO−; common commercial forms include sodium hypochlorite (NaClO) and calcium hypochlorite (Ca(OCl)2). In water, hypochlorite exists in equilibrium with hypochlorous acid: ClO− + H2O ⇌ HOCl + OH−, with HOCl being the more effective disinfectant. The relative amounts depend on pH; at pH below about 7.5 HOCl dominates, while at higher pH ClO− dominates. HOCl’s higher reactivity makes it the principal microbial oxidant in typical drinking-water disinfection.

Sodium hypochlorite solutions are widely used as liquid bleaches and sanitizers; calcium hypochlorite is sold as a solid bleaching powder and is common in water treatment and sanitizing products. Other metal hypochlorites exist but are less common. Production traditionally arises from the chlor-alkali process to generate chlorine, followed by reaction with sodium or calcium hydroxide to form hypochlorite.

Applications include sanitization of drinking water, swimming pools, and surfaces; disinfection in food processing; bleaching of paper, textiles, and cotton; and as an oxidizing agent in organic synthesis. Safety concerns center on strong oxidizing properties, corrosivity, and potential release of chlorine gas if the material is acidified or heated. Storage requires compatible materials and protection from heat; mixing with ammonia, acids, or organic compounds can generate hazardous byproducts.

Environmental impact includes the formation of disinfection byproducts when hypochlorites react with natural organic matter. Regulations govern concentration and handling in consumer products and municipal water treatment.