Chloric acid
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| Names | |
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| Other names
Chloric(V) acid
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| Identifiers | |
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3D model (Jmol)
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| ChemSpider | |
| ECHA InfoCard | 100.029.303 |
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| Properties | |
| HClO3 | |
| Molar mass | 84.45914 g mol−1 |
| Appearance | colourless solution |
| Density | 1 g/mL, solution (approximate) |
| >40 g/100 ml (20 °C) | |
| Acidity (pKa) | ca. −1 |
| Structure | |
| pyramidal | |
| Hazards | |
| Main hazards | Oxidant, Corrosive |
| Safety data sheet | See: data page |
| NFPA 704 | |
| Related compounds | |
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Other anions
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bromic acid iodic acid |
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Other cations
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ammonium chlorate sodium chlorate potassium chlorate |
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Related compounds
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hydrochloric acid hypochlorous acid chlorous acid perchloric acid |
| Supplementary data page | |
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Refractive index (n), Dielectric constant (εr), etc. |
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Thermodynamic
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Phase behaviour solid–liquid–gas |
| UV, IR, NMR, MS | |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |
Chloric acid, HClO3, is an oxoacid of chlorine, and the formal precursor of chlorate salts. It is a strong acid (pKa ≈ −1) and oxidizing agent.
Chloric acid is thermodynamically unstable with respect to disproportionation.
Chloric acid is stable in cold aqueous solution up to a concentration of approximately 30%, and solution of up to 40% can be prepared by careful evaporation under reduced pressure. Above these concentrations, chloric acid solutions decompose to give a variety of products, for example:
Chloric acid is a powerful oxidizing agent. Most organics and flammables will deflagrate on contact.
It can be prepared by the reaction of sulfuric acid with barium chlorate, the insoluble barium sulfate being removed by precipitation:
Another method is the heating of hypochlorous acid, producing chloric acid and hydrogen chloride:
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