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}} In chemistry, hypochlorite is an ion composed of chlorine and oxygen, with the chemical formula ClO−. It can combine with a number of counter ions to form hypochlorites, which may also be regarded as the salts of hypochlorous acid. Common examples include sodium hypochlorite (household bleach) and calcium hypochlorite (bleaching powder, swimming pool "chlorine"). Hypochlorites are frequently quite unstable in their pure forms and for this reason are normally handled as aqueous solutions. Their primary applications are as bleaching, disinfection and water treatment agents but they are also used in chemistry for chlorination and oxidation reactions. ==Preparation== A variety of hypochlorites can be formed by a disproportionation reaction between chlorine gas and metal hydroxides. The reaction must be performed at close to room temperature, as further oxidation will occur at higher temperatures leading to the formation of chlorates. This process is widely used for the industrial production of sodium hypochlorite (NaClO) and calcium hypochlorite (Ca(ClO)2). :Cl2 + 2 NaOH → NaCl + NaClO + H2O :2 Cl2 + Ca(OH)2 → CaCl2 + Ca(ClO)2 + H2O Large amounts of sodium hypochlorite are also produced electrochemically via an un-separated chloralkali process. In this process brine is electrolyzed to form which dissociates in water to form hypochlorite. This reaction must be run in non-acidic conditions to prevent chlorine gas from bubbling out of solution: :2 → + 2 e− : + ↔ + + Small amounts of more unusual hypochlorites may also be formed by a salt metathesis reaction between calcium hypochlorite and various metal sulfates. This reaction is performed in water and relies on the formation of insoluble calcium sulfate, which will precipitate out of solution, driving the reaction to completion. : Ca(ClO)2 + MSO4 → M(ClO)2 + CaSO4 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Hypochlorite」の詳細全文を読む スポンサード リンク
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