chlorates

Chlorates are salts and esters derived from chloric acid (HClO3). The chlorate ion, ClO3-, features chlorine in the +5 oxidation state. The most common chlorate salts are sodium chlorate (NaClO3) and potassium chlorate (KClO3), though many metal chlorates are known. Chlorates are strong oxidizing agents and are widely used as industrial oxidizers.

Properties of chlorates include high solubility in water for many salts and a tendency to decompose when heated, releasing oxygen and, in some cases, chlorine dioxide. While relatively stable at room temperature, chlorates can form explosive mixtures with organic materials or reducing agents, and they should be handled with care. Acids can promote the release of chlorine dioxide from chlorate solutions, a toxic oxidizing gas.

Production and applications: Chlorates are typically produced by electrolysis of sodium chloride solutions to generate sodium chlorate, an intermediate in various processes. Industrially, chlorates have been used in herbicides (for example, sodium chlorate), in paper and textile bleaching, and historically in matches and fireworks. They also serve as oxidizing agents in chemical synthesis and various laboratory applications. Due to safety concerns, many uses have declined or become tightly regulated in favor of less hazardous alternatives.

Safety and handling: Chlorates pose health and safety risks if ingested, inhaled, or subjected to heat or friction. They can cause skin and eye irritation and, in higher exposures, more serious toxic effects. They react vigorously with reducing agents and organic materials, and acids can generate chlorine dioxide gas. Proper storage in cool, dry conditions and separation from combustibles and reducing substances is essential.