Ammonium iodide

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Ammonium iodide
The ammonium cation
The ammonium cation
The iodide anion
The iodide anion
ball-and-stick model of an ammonium cation (left) and an iodide anion (right)
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.031.548 Edit this at Wikidata
UNII
  • InChI=1S/HI.H3N/h1H;1H3 checkY
    Key: UKFWSNCTAHXBQN-UHFFFAOYSA-N checkY
  • InChI=1/HI.H3N/h1H;1H3
    Key: UKFWSNCTAHXBQN-UHFFFAOYAU
  • [I-].[NH4+]
Properties
NH4I
Molar mass 144.94 g/mol
Appearance White crystalline powder
Density 2.51 g/cm3
Melting point 551 °C (1,024 °F; 824 K) (sublimes)
Boiling point 235 °C (455 °F; 508 K) (in vacuum)
155 g/100 mL (0 °C)
172 g/100 mL (20 °C)
250 g/100 mL (100 °C)
-66.0·10−6 cm3/mol
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point Non-flammable
Related compounds
Other anions
 Ammonium fluoride
Ammonium chloride
Ammonium bromide
Other cations
 Sodium iodide
Potassium iodide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Ammonium iodide is the chemical compound NH4I. It is used in photographic chemicals and some medications.[1] It can be prepared by the action of hydroiodic acid on ammonia. It is easily soluble in water, from which it crystallizes in cubes. It is also soluble in ethanol. It gradually turns yellow on standing in moist air, owing to decomposition with liberation of iodine.[1]

Preparation

Ammonium iodide can be made in lab by reacting ammonia or ammonium hydroxide with hydroiodic acid or hydrogen iodide gas:

NH3 + HI → NH4I
NH4OH + HI → NH4I + H2O

It is also formed by the decomposition of ammoniated triiodoamine (an explosive).

References

  1. ^ a b Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
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