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Copyright © Tarek Kakhia. All rights reserved. http://tarek.kakhia.org 3 . Acidity Perchloric acid is a superacid, and one of the strongest Brønsted - Lowry acids. Its pKa is −10 . Anhydrous per chloric acid is an oily liquid. It forms a series of at least five hydrates, several of which have been characterized crystallographically. The dihydrate is representative: the solid consists of the per chlorate anion linked to H2O and H3O+ centers via hydrogen bonds. Per chloric acid forms an azeotrope with water, consisting of about 72.5 % per chloric acid. This form of the acid is stable indefinitely and is commercially available. Such solutions are hygroscopic, that is, if left unsealed, concentrated acid dilutes itself by absorbing water from the air. 4 . Laboratory preparation The concentrated acid can be prepared by distillation of a solution of sodium per chlorate in concentrated sulfuric acid. Na ClO4 + H2SO4 → Na HSO4 + H ClO4 In a related method, barium per chlorate reacts with dilute sulfuric acid to precipitate barium sulfate, leaving per chloric acid. It also can be made by mixing nitric acid with ammonium per chlorate. The reaction gives nitrous oxide and per chloric acid due to a concurrent reaction involving the ammonium ion. 5 . Safety Anhydrous and monohydrated perchloric acid are explosive, but the usual aqueous solutions are stable in the absence of organic compounds. It is very corrosive to skin and eyes. Upon contact with perchloric acid, organic materials such as cloth and wood ignite. Salts of perchloric acid are also powerful oxidizers that can be explosive. Perchlorate salts tend to be more stable than their chlorate counterparts, which has led to their increased use in pyrotechnic compositions due to safety concerns. 42PDF Image | Chlorine Characteristics
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