Iodic acid

Chembox new
Name = Iodic acid
ImageFile = Iodic-acid-2D.png ImageName = Iodic acid
ImageFileL1 = Iodic-acid-3D-balls.png ImageNameL1 = Ball-and-stick model of iodic acid
ImageFileR1 = Iodic-acid-3D-vdW.png ImageNameR1 = Space-filling model of iodic acid
OtherNames = Iodic(V) acid
Section1 = Chembox Identifiers
CASNo = 7782-68-5
Section2 = Chembox Properties
Formula = HIO₃
MolarMass = 175.91 g/mol
Appearance = white solid
Density = 4.62 g/cm³, solid
Solubility = 269 g/100 ml (20 °C)
MeltingPt = 110 °C
BoilingPt =
pKa = 0.75
Section3 = Chembox Structure
MolShape =
Dipole =
Section7 = Chembox Hazards
ExternalMSDS =
EUClass = not listed
FlashPt = non flammable
Section8 = Chembox Related
OtherAnions = Hydriodic acid
Periodic acid
OtherCations = Potassium iodate
Function = oxoacids
OtherFunctn = Chloric acid
Bromic acid
OtherCpds = Iodine pentoxide

Iodic acid, HIO₃, can be obtained as a white solid. It dissolves in water very well, but it also exists in the pure state, as opposed to chloric acid or bromic acid. Iodic acid contains iodine in the oxidation state +5 and it is one of the most stable oxo-acids of the halogens in its pure state. When iodic acid is carefully heated, then it loses water, and iodine pentoxide remains behind. On stronger heating, the iodine pentoxide further decomposes, giving a mix of iodine, oxygen and lower oxides of iodine.

Preparation

Iodic acid can be produced by oxidizing I₂ with chlorine in an aqueous solution.

Properties

Iodic acid is a relatively strong acid with a p"K"_a of 0.75. It is strongly oxidizing in acidic solution, less so in basic solution. When iodic acid acts as oxidizer, then the product of the reaction is either iodine, or iodide ion. Under some special conditions (very low pH and high concentration of chloride ion, e.g. in concentrated hydrochloric acid), iodic acid is reduced to iodine trichloride, a golden yellow compound in solution and no further reduction occurs. In the absence of chloride ions, when there is an excess amount of reductor, then all iodate is converted to iodide ion. When there is an excess amount of iodate, then part of the iodate is converted to iodine.

Uses

Iodic acid is used as a standard strong acid in analytical chemistry. It may be used to standardize solutions of both weak and strong bases, with methyl red or methyl orange as the indicator.

References