Chloric acid

Chloric acid
Names
Other names
Chloric(V) acid
Identifiers
7790-93-4
ChemSpider 18513
Jmol interactive 3D Image
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
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
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
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.

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:

8HClO3 → 4HClO4 + 2H2O + 2Cl2 + 3 O2
3HClO3 → 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 → 2HClO3 + BaSO4

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

3HClO → HClO3 + 2 HCl

See also

References

    This article is issued from Wikipedia - version of the Monday, November 16, 2015. The text is available under the Creative Commons Attribution/Share Alike but additional terms may apply for the media files.