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|Section2= |Section3= |Section4= |Section7= |Section8= }} Potassium chlorate is a compound containing potassium, chlorine and oxygen atoms, with the molecular formula KClO3. In its pure form, it is a white crystalline substance. It is the most common chlorate in industrial use. It is used * as an oxidizing agent, * to prepare oxygen, * as a disinfectant, * in safety matches, * in explosives and fireworks, * in cultivation, forcing the blossoming stage of the Longan tree, causing it to produce fruit in warmer climates. ==Production== On the industrial scale, potassium chlorate is produced by the Liebig process: passing chlorine into hot calcium hydroxide, subsequently adding potassium chloride: .〔Реми, Г. Курс неорганической химиию, т. 1/Перевод с немецкого под ред. А. В. Новосёловой. Москва:Мир, 1972.- с. 770//(translated from:) Heinrich Remy. Lehrbuch der anorganischen Chemie. XI Auflage. Band 1. Leipzig:Geest & Portig K.-G., 1960.〕 : 6Ca(OH)2 + 6Cl2 -> Ca(ClO3)2 + 5CaCl2 + 6H2O : Ca(ClO3)2 + 2KCl -> 2KClO3 + CaCl2 The electrolysis of KCl in aqueous solution is also used sometimes, in which the chloride ions formed at the anode react with KOH ''in situ''. The low solubility of KClO3 in water causes the salt to conveniently isolate itself from the reaction mixture by simply precipitating out of solution. Potassium chlorate can be produced in small amounts by disproportionation in a sodium hypochlorite solution followed by metathesis reaction with potassium chloride: :3 NaClO → 2NaCl + NaClO3 :KCl + NaClO3 → NaCl + KClO3 It can also be produced by passing chlorine gas into a hot solution of caustic potash:〔Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0-07-049439-8〕 :3 Cl2(g) + 6 KOH(aq) → KClO3(aq) + 5 KCl(aq) + 3 H2O(l) 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「potassium chlorate」の詳細全文を読む スポンサード リンク
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