1. Properties

2. Hazards

3. Production

4. See also

5. References

Chloric acid, HClO₃, is an oxoacid of chlorine, and the formal precursor of chlorate salts. It is a strong acid (pK_a ≈ −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:

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

• Chlorate
• Hypochlorous acid
• Chlorous acid
• Perchloric acid
• Oxidizing acid

References

• {{cite encyclopedia |editor= R. Bruce King|encyclopedia= Encyclopedia of Inorganic Chemistry|title= Chloric acid|year= 1994|publisher= Wiley|volume= 2|location= Chichester|isbn= 0-471-93620-0|page= 658}}

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