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|Section2= |Section7= |Section8= }} Perchloric acid is an inorganic compound with the formula HClO4. Usually found as an aqueous solution, this colorless compound is a stronger acid than sulfuric and nitric acid. It is a powerful oxidizer when hot, but its aqueous solutions up to approximately 70% and room temperature are generally safe, only showing strong acid features and no oxidizing properties. Perchloric acid is useful for preparing perchlorate salts, especially ammonium perchlorate, an important rocket fuel. Overall, perchloric acid is dangerously corrosive and readily forms potentially explosive mixtures. ==Production== Perchloric acid is produced industrially by two routes. The traditional method exploits the high aqueous solubility of sodium perchlorate (209 g/100 mL of water at room temperature). Treatment of such solutions with hydrochloric acid gives perchloric acid, precipitating solid sodium chloride: :NaClO4 + HCl → NaCl + HClO4 The concentrated acid can be purified by distillation. The alternative route, which is more direct and avoids salts, entails anodic oxidation of aqueous chlorine at a platinum electrode.〔Helmut Vogt, Jan Balej, John E. Bennett, Peter Wintzer, Saeed Akbar Sheikh, Patrizio Gallone "Chlorine Oxides and Chlorine Oxygen Acids" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. .〕〔; (German patent DE1031288B ); (US patent US2846383A )〕 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「perchloric acid」の詳細全文を読む スポンサード リンク
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