Chloric acid

Chloric acid, HClO3, is an oxoacid of chlorine, and the formal precursor of chlorate salts. It is a strong acid (pKa ≈ −2,7) and oxidizing agent.

Chloric acid
Names
Other names
Chloric(V) acid
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.303
EC Number
  • 232-233-0
PubChem CID
UNII
UN number 2626
CompTox Dashboard (EPA)
Properties
Chemical formula
 HClO3
Molar mass 84.45914 g mol−1
Appearance colourless solution
Density 1 g/mL, solution (approximate)
Solubility in water
 >40 g/100 ml (20 °C)
Acidity (pKa) ~ −1
Conjugate base Chlorate
Structure
Molecular shape
 pyramidal
Hazards
Main hazards Oxidant, Corrosive
Safety data sheet See: data page
GHS pictograms
GHS Signal word Danger
GHS hazard statements
 H271, H314
GHS precautionary statements
 P210, P220, P221, P260, P264, P280, P283, P301+330+331, P303+361+353, P304+340, P305+351+338, P306+360, P310, P321, P363, P370+378, P371+380+375, P405, P501
NFPA 704 (fire diamond)
0
3
2
OX
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
Supplementary data page
Structure and
properties
 Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
Spectral data
 UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Properties

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

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

Production

It can be prepared by the reaction of sulfuric acid with barium chlorate, the insoluble barium sulfate being removed by precipitation:

Ba(ClO3)2 + H2SO4 → 2 HClO3 + BaSO4

Another method is the heating of hypochlorous acid, producing chloric acid and hydrogen chloride:

3 HClO → HClO3 + 2 HCl

See also

References
    • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
    • R. Bruce King, ed. (1994). "Chloric acid". Encyclopedia of Inorganic Chemistry. 2. Chichester: Wiley. p. 658. ISBN 0-471-93620-0.
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