Arsenic acid


Arsenic acid is the chemical compound with the formula H3AsO4. More descriptively written as AsO3, this colorless acid is the arsenic analogue of phosphoric acid. Arsenate and phosphate salts behave very similarly. Arsenic acid as such has not been isolated, but is only found in solution, where it is largely ionized. Its hemihydrate form does form stable crystals. Crystalline samples dehydrate with condensation at 100 °C.

Properties

It is a tetrahedral species of idealized symmetry C3v with As-O bond lengths ranging from 1.66 to 1.71 Å.
Being a triprotic acid, its acidity is described by three equilibria:
These Ka values are close to those for phosphoric acid. The highly basic arsenate ion is the product of the third ionization. Unlike phosphoric acid, arsenic acid is an oxidizer, as illustrated by its ability to convert iodide to iodine.

Preparation

Arsenic acid is prepared by treating arsenic trioxide with concentrated nitric acid. Dinitrogen trioxide is produced as a by-product.
The resulting solution is cooled to give colourless crystals of the hemihydrate H3AsO4·H2O, although the dihydrate H3AsO4·2H2O is produced when crystallisation occurs at lower temperatures.

Other methods

Arsenic acid is slowly formed when arsenic pentoxide is dissolved in water, and when meta- or pyroarsenic acid is treated with cold water. Arsenic acid can also be prepared directly from elemental arsenic by moistening it and treating with ozone.

Applications

Commercial applications of arsenic acid are limited by its toxicity. It is a precursor to a variety of pesticides. It has found occasional use as a wood preservative, a broad-spectrum biocide, a finishing agent for glass and metal, and a reagent in the synthesis of some dyestuffs and organic arsenic compounds.

Safety

Arsenic acid is extremely toxic and carcinogenic, like all arsenic compounds. It is also corrosive. The in rabbits is 6 mg/kg.