Ammonium iodate

Structural formula
General
Surname	Ammonium iodate
Molecular formula	NH 4 IO 3
Brief description	colorless and odorless solid
External identifiers / databases
CAS number 13446-09-8 EC number 236-592-4 ECHA InfoCard 100.033.252 Wikidata Q4202633
properties
Molar mass	192.94 g mol −1
Physical state	firmly
density	3.309 g cm −3
Melting point	Decomposition from 150 ° C
solubility	20.6 g l −1 at 20 ° C
safety instructions
GHS labeling of hazardous substances danger H and P phrases H: 272-315-319-335 P: 221-210-220-261-280-305 + 351 + 338-304 + 340-362-405-501
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Ammonium iodate is the ammonium salt of iodic acid . It is a white salt that is sparingly soluble in water and - like all iodates - has an oxidizing effect.

Manufacturing

Ammonium iodate can be made by neutralizing iodic acid with ammonia.

${\displaystyle \mathrm {NH_{3}+HIO_{3}\longrightarrow NH_{4}IO_{3}} }$

It can also be precipitated from an iodate solution with an ammonium salt.

${\displaystyle \mathrm {2\ KIO_{3}+(NH_{4})_{2}SO_{4}\longrightarrow 2\ NH_{4}IO_{3}+K_{2}SO_{4}} }$

properties

Ammonium iodate dissolves poorly in cold and moderately in warm water. It contains an oxidizing anion and a reducing cation, so it decomposes to nitrogen, oxygen, iodine and water at 150 ° C.

${\displaystyle \mathrm {2\ NH_{4}IO_{3}\longrightarrow N_{2}+O_{2}+I_{2}+4\ H_{2}O} }$

From 60 ° C the reaction can be sustained without an external heat source. With 10% potassium dichromate or copper (II) chloride as a catalyst, ammonium iodate can burn at room temperature, and the development of purple-colored iodine vapor can be observed.

safety instructions

Ammonium iodate is a strong oxidizing agent and can react violently with combustible materials.

Individual evidence

1. ↑ ^{a b c d e f g} data sheet Ammonium iodate, 99% at AlfaAesar, accessed on October 28, 2016 ( PDF )(JavaScript required) .
2. ↑ ^{a b c} A. A. Shidlovskiy: COMBUSTION OF THE INORGANIC SALTS AMMONILM IODATE AND HYDROXYLAMINE SULFATE , Zhurnal Prikladnoy Khimii, Vol. 35, No. 3, 1962, pp. 511-516.
3. ^ Brockhaus ABC Chemie , VEB FA Brockhaus Verlag Leipzig 1965, p. 604.