Hypochlorite

Hypochlorite is the anion ClO⁻, with chlorine in the +1 oxidation state, and the salts containing it. It is a strong oxidizing agent used in bleaching and disinfection.

Hypochlorous acid: A weak acid, HOCl, formed when hypochlorite accepts a proton in water. Its balance with ClO⁻ governs hypochlorite solutions’ activity and speciation.
Sodium hypochlorite: The sodium salt of hypochlorite, commonly used in household bleach and disinfectants. It is the most widely encountered hypochlorite salt.
Oxidation state: A formal accounting value used to track electron distribution in chemical compounds and ions. The +1 value identifies chlorine’s electron accounting in ClO⁻.
Chlorite: The anion ClO₂⁻, in which chlorine has the +3 oxidation state. Chlorite contains one more oxygen atom and chlorine at a higher oxidation state.
Oxidation–reduction reaction: A chemical reaction involving electron transfer and changes in oxidation state. Hypochlorite oxidizes many substances while chlorine is reduced.
Calcium hypochlorite: A calcium salt of hypochlorite used as a concentrated solid disinfectant and bleaching agent. Its solid form is widely used to treat swimming pools and drinking water.
Oxoanion: A negatively charged polyatomic ion containing oxygen bonded to another element. ClO⁻ belongs to the chlorine oxoanion family.
Chlorate: The anion ClO₃⁻, in which chlorine has the +5 oxidation state. Chlorate is a more oxidized chlorine oxoanion and a possible disproportionation product.
Chlorine disproportionation: A reaction in which chlorine in one oxidation state forms products with higher and lower oxidation states. Hypochlorite can disproportionate into chloride and chlorate, especially in concentrated or warm solutions.
Water chlorination: Disinfection of water by adding chlorine-containing agents that form active chlorine species. Hypochlorite salts supply disinfecting chlorine in water treatment.

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