Chloric acid

Chloric acid
Names
	Other names Chloric(V) acid
Identifiers
CAS Number	7790-93-4;
3D model (JSmol)	Interactive image;
ChemSpider	18513;
ECHA InfoCard	100.029.303
EC Number	232-233-0;
PubChem CID	19654;
UNII	Z0V9L75H3K;
UN number	2626
CompTox Dashboard (EPA)	DTXSID1047449 ;
	InChI InChI=1/ClHO3/c2-1(3)4/h(H,2,3,4) Key: XTEGARKTQYYJKE-UHFFFAOYAG;
	SMILES O[Cl 2]([O-])[O-];
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)	−2.7
Conjugate base	Chlorate
Structure
Molecular shape	pyramidal
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Oxidant, Corrosive
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H271, H314
Precautionary statements	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)	3 0 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
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Chloric acid, H Cl O₃, is an oxoacid of chlorine, and the formal precursor of chlorate salts. It is a strong acid (pK_a ≈ −2.7) and an 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:

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

References

^ 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)

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. Vol. 2. Chichester: Wiley. p. 658. ISBN 0-471-93620-0.

[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)

[1]

Properties

Hazards

Production

See also

References