Abstract: In 1906, Van Wyk suggested that the anhydrous acid did not exist alone but was always associated with chlorine heptoxide and perchloric acid monohydrate in equilibrium. This chapter reviews the evidence for and against this suggestion. Perchloric acid is one of the strongest acids and contains more oxygen (63.7%) than any other common acid. However, its oxidizing power depends on both concentration and temperature. The perchlorate ion itself shows no oxidizing properties in solution. The chapter highlights the preparation of perchlorate with anhydrous acid, hydrated acid, and deuteroperchloric acid. Perchloric acid, 60% and 72%, is prepared on an industrial scale either or by anodic oxidation of hydrochloric acid or a chlorate. Physical properties and chemical properties of perchloric acid have been highlighted in the chapter. Perchloric acid is one of the strongest acids known. Its solution in fluorosulfonic acid is one of the few cases where it is believed not to ionize to form the perchlorate ion. Under the chemical properties of perchloric acid, the chapter discusses the nature of mixed acid systems and the explosion hazard concerned with the use of anhydrous acid. Some uses of the perchloric acid have been discussed. Perchloric acid is used widely in analytical laboratories and in industry as a solvent for many materials, because it does not readily form complexes, and for the destruction of organic matter. Other applications have included extraction of iron compounds and ores by perchloric acid solution.
Publication Year: 1966
Publication Date: 1966-01-01
Language: en
Type: book-chapter
Indexed In: ['crossref']
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Cited By Count: 31
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