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• Physical Properties

  White stable crystalline solid; rhombohedral crystals; occurs in two forms: the normal HIO3, and pyroiodic acid HI3O8. ;

• Uses

  Aqueous solutions of iodic acid serve as strong oxidizing agents. The acid also is used in redox titrations. ;

• Preparation

  Iodic acid may be prepared by the reaction of sulfuric acid with barium iodate. The solution is filtered to remove barium sulfate and then crystallized to obtain iodic acid:
  Ba(IO3)2 + H2SO4 → BaSO4 + 2HIO3
  It also may be produced by oxidation of iodine with concentrated nitric acid:
  3I2 + 10HNO3 → 6HIO3 + 10NO + 2H2O
  Also, iodic acid may be obtained by oxidation of iodine with chlorine in dilute acidic solutions:
  I2 + 5Cl2 + 6H2O → 2HIO3 + 10HCl
  Another method of preparation involves oxidation of iodine with hydrogen peroxide:
  I2 + 5H2O2 → 2HIO3 + 4H2O
  It also may be prepared by treating hypoiodous acid with a base:
  3HIO + 2OH¯ → HIO3 + 2H2O + I¯
  Hypoiodous acid may be obtained by alkaline hydrolysis of iodine at pH 12:
  I2 + H2O → HIO + H+ + I¯
  Iodic acid dehydrates to iodine pentaoxide when heated at 180°C:
  2HIO3 → I2H5 + H2O
  Iodic acid is a relatively weak monoprotic acid, the Ka value at 25°C is 1.6 x 10–1. Several species have been detected in concentrated aqueous solutions, which include IO3¯, H+, HIO3, (HIO3)2 and (HIO3)3. Its solution turns blue litmus red and then bleaches the litmus paper because of its strong oxidizing properties.
  When heated with potassium iodate, potassium hydrogen iodate is formed:
  HIO3 + KIO3 → KH(IO3)2
  An aqueous solution of iodic acid is a strong oxidizing agent. It liberates iodine from iodides:
  IO3¯ + 5I¯ + 6H+ → 3I2 + 3H2O or,
  HIO3 + 5HI → 3I2 + 3H2O
  In an aqueous solution, iodic acid oxidizes hydrogen sulfide to sulfur:
  2HIO3 + 5H2S → I2 + 6H2O + 5S
  The solid iodic acid reacts vigorously with sulfur, phosphorus and other nonmetals. ;

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