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Chloric acid

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Chloric acid
Chloric acid
Chloric acid
Names
Other names
Chloric(V) acid
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.303 Edit this at Wikidata
EC Number
  • 232-233-0
UNII
UN number 2626
  • InChI=1/ClHO3/c2-1(3)4/h(H,2,3,4)
    Key: XTEGARKTQYYJKE-UHFFFAOYAG
  • O[Cl+2]([O-])[O-]
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) −2.7[1]
Conjugate base Chlorate
Structure
pyramidal
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
Oxidant, Corrosive
GHS labelling:
GHS03: OxidizingGHS05: Corrosive
Danger
H271, H314
P210, P220, P221, P260, P264, P280, P283, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P306+P360, P310, P321, P363, P370+P378, P371+P380+P375, P405, P501
NFPA 704 (fire diamond)
Related compounds
Other anions
bromic acid
iodic acid
Other cations
ammonium chlorate
sodium chlorate
potassium chlorate
Related compounds
hydrochloric acid
hypochlorous acid
chlorous acid
perchloric acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Chloric acid, HClO3, is an oxoacid of chlorine, and the formal precursor of chlorate salts. It is a strong acid (pKa ≈ −2.7) and an oxidizing agent.

Properties

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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:

8 HClO3 → 4 HClO4 + 2 H2O + 2 Cl2 + 3 O2
3 HClO3 → HClO4 + H2O + 2 ClO2

Hazards

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Chloric acid is a powerful oxidizing agent. Most organics and flammables will deflagrate on contact.[citation needed]

Production

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It may be produced from barium chlorate through its reaction with sulfuric acid, which results in a solution of chloric acid and insoluble barium sulfate precipitate:[2]

Ba(ClO3)2 + H2SO4 → 2 HClO3 + BaSO4

The chlorate must be dissolved in boiling water and the acid should be somewhat diluted in water and heated before mixing.

Another method which can be used to produce solutions up to 10% concentration is by the use of cation exchange resins and a soluble salt such as NaClO3, where the Na+ cation will exchange with H+.[2]

Another method is the heating of hypochlorous acid, producing chloric acid and hydrogen chloride:[citation needed]

3 HClO → HClO3 + 2 HCl

Any way it is produced, the acid may be concentrated up to 40% in a vacuum dessicator over H2SO4.[2]

See also

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References

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  1. ^ Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (2007). Lehrbuch der anorganischen Chemie (in German). Berlin. ISBN 978-3-11-017770-1. OCLC 180963521.{{cite book}}: CS1 maint: location missing publisher (link)
  2. ^ a b c Brauer, Georg; Schmeisser, M. (1963). "5. Chlorine, Bromine, Iodine". In Riley, Reed F. (ed.). Handbook of Preparative Inorganic Chemistry (2nd ed.). New York, London: Academic Press. pp. 312–313. ISBN 9780121266011. Retrieved 6 December 2024.

Additional Information

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