klorat

Klorat, or chlorate, refers to the chlorate ion ClO3− and to salts that contain it, such as potassium chlorate (KClO3) and sodium chlorate (NaClO3). The chlorate ion carries chlorine in the +5 oxidation state and adopts a roughly tetrahedral arrangement around chlorine. Chlorates are typically highly soluble in water and act as strong oxidizers.

Industrial production of chlorates usually involves the oxidation of chloride-containing solutions, such as by electrolysis of brine or oxidation of hypochlorite under controlled conditions. They are used because of their oxidative power in applications ranging from chemical synthesis to bleaching processes.

Common uses include bleaching agents in the paper and textile industries, components in fireworks and pyrotechnics, and historic roles in herbicides and disinfectants. Sodium chlorate and potassium chlorate are the best-known examples, each with distinct industrial applications and regulatory considerations.

Safety and handling are important due to their oxidizing nature. Chlorates can react violently with organic materials or reducing agents and may decompose upon heating, releasing oxygen or chlorine dioxide. Acidification of chlorate solutions can generate chlorine dioxide, a hazardous gas. Ingestion or prolonged exposure can be toxic, potentially causing methemoglobinemia and other adverse effects. Because of these hazards, chlorates are subject to strict storage, handling, and regulatory controls in many jurisdictions.

See also: chlorates in chemistry, chlorite, hypochlorite, bleaching agents.