chlorate

Chlorate refers to the chlorate ion, ClO3−, an oxyanion of chlorine in oxidation state +5. It forms salts including sodium chlorate, potassium chlorate, and ammonium chlorate. The corresponding parent acid is chloric acid, HClO3. In aqueous solution, chlorate exists as ClO3− and combines with various cations to form solid chlorate salts.

Chlorates are strong inorganic oxidizers. They are typically crystalline, highly soluble salts at room temperature. They are stable under normal conditions but can decompose exothermically when heated or when in contact with reducing agents or organic material. Acidification or contact with fuels can release chlorine dioxide, a toxic oxidant, making handling hazardous.

Production and occurrence: Sodium chlorate is produced industrially by electrolysis of concentrated sodium chloride brine in the chlorate process, which oxidizes chloride to chlorate at the anode. Chlorates are also prepared by neutralizing chloric acid. They occur mainly as synthetic compounds; trace chlorate can arise as byproducts in water treatment and industrial processes.

Applications: Chlorates are used as bleaching agents in pulp and paper and textiles; as oxidizers in fireworks, pyrotechnics, and matches; some chlorates have been used as herbicides and in chemical synthesis and disinfection.

Safety and environmental considerations: Chlorates are strong oxidizers and can react violently with fuels and reducing agents. They pose fire and explosion hazards, especially when contaminated with organic matter or metals. In the environment, chlorates can persist and may be reduced to chlorite; regulatory attention is given to drinking water and wastewater.