|Jmol-3D images||Image 1|
|Molar mass||84.45914 g mol−1|
|Density||1 g/mL, solution (approximate)|
|Solubility in water||>40 g/100 ml (20 °C)|
|Acidity (pKa)||ca. −1|
|Main hazards||Oxidant, Corrosive|
|Other anions||bromic acid
|Other cations||ammonium chlorate
|Related compounds||hydrochloric acid
|Supplementary data page|
|n, εr, etc.|
Solid, liquid, gas
|Spectral data||UV, IR, NMR, MS|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
- Ba(ClO3)2 + H2SO4 → 2HClO3 + BaSO4
- 3HClO → HClO3 + 2 HCl
It is also produced by the reaction of sulfuric acid with potassium chlorate in the combustion of sugar using potassium chlorate, sulfuric acid, and sugar.
It 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, and on warming, chloric acid solutions decompose to give a variety of products, for example:
- 8HClO3 → 4HClO4 + 2H2O + 2Cl2 + 3 O2
- 3HClO3 → HClO4 + H2O + 2 ClO2
The decomposition is controlled by kinetic factors: indeed, chloric acid is never thermodynamically stable with respect to disproportionation.
Chloric acid is a dangerously powerful oxidizing agent and will cause most organics and flammables to deflagrate on contact. For example a mixture of potassium chlorate and sugar will burn when concentrated sulfuric acid is added due to chloric acid production. Because sulfur tends to contain acidic impurities, it will form highly unstable mixtures with potassium chlorate due to chloric acid being produced.
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.
- R. Bruce King, ed. (1994). "Chloric acid". Encyclopedia of Inorganic Chemistry 2. Chichester: Wiley. p. 658. ISBN 0-471-93620-0.
|This inorganic compound–related article is a stub. You can help Wikipedia by expanding it.|