Iodic acid

Chemical properties

colorless, rhomb crystal(s) or white, crystal(s) powder(s); darkens on exposure to light; it is a moderately strong acid; used in analytical chemistry and in medicine [HAW93] [MER06]

Physical properties

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, it dehydrates to iodine pentoxide. On subsequent heating, the iodine pentoxide further decomposes, giving a mixture of iodine, oxygen and lower oxides of iodine.
Iodic acid can be produced by oxidizing I2 with chlorine in an aqueous solution. Iodic acid can be used to synthesize sodium or potassium iodate salts (which are used in salt as a source of iodine in the human body.

The Uses of Iodic acid

Iodic acid is used in analytical chemistry laboratories to standardize solutions of both weak and strong bases using methyl red or methyl orange as the indicator. It acts as a key starting material to synthesize sodium or potassium iodate, thereby increasing the iodine content of salt.

The Uses of Iodic acid

A strong acid in analytical chemistry.

What are the applications of Application

Iodic acid is a strong acid in analytical chemistry

Definition

iodic acid: Any of various oxoacids of iodine, such as iodic(V) acid and iodic(VII) acid. When used without an oxidation state specifled, the term usually refers to iodic(V) acid (HIO₃).

Preparation

Iodic acid may be prepared by the reaction of sulfuric acid with bariumiodate. The solution is filtered to remove barium sulfate and then crystallizedto 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 diluteacidic solutions:
I₂ + 5Cl₂ + 6H₂O → 2HIO₃ + 10HCl
Another method of preparation involves oxidation of iodine with hydrogenperoxide:
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 1.6x10-1. Several species have been detected in concentrated aqueous solutions,which include IO3^-, H⁺, HIO₃, (HIO₃)₂ and (HIO₃)₃. Its solution turns blue lit-mus red and then bleaches the litmus paper because of its strong oxidizingproperties.
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 non-metals.

General Description

Iodic acid is the hydrated form of I₂O₅. Reaction of iodic acid with hydrogen iodide has been described by electrolytic dissociation theory. Combustion of mixture of chromic, iodic, sulfuric and phosphoric acids has been proposed. Its Raman spectra have been recorded. Vibrational assignment of IO₃^- has been evaluated.

Hazard

Toxic by ingestion, strong irritant to eyes and skin.

Purification Methods

Dissolve iodic acid in the minimum volume of hot dilute HNO3, filter and evaporate in a vacuum desiccator until crystals are formed. Collect the crystals and wash them with a little cold H2O and dry them in air in the dark. It is soluble in H2O: 269g/100mL at 20o and 295g/100mL at 40o. It is soluble in dilute EtOH and darkens on exposure to light. It is converted to HIO3.I2O5 on heating at 70o, but at 220o complete conversion to HIO3 occurs. [Lamb et al. J Am Chem Soc 42 1636 1920, Bray & Caulkins J Am Chem Soc 53 44 1931.]