Ammonium iodide
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| ECHA InfoCard | 100.031.548  | ||
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| Properties | |||
Chemical formula | 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) | ||
Solubility in water | 155 g/100 mL (0 °C) 172 g/100 mL (20 °C) 250 g/100 mL (100 °C) | ||
Magnetic susceptibility (χ) | −66.0×10−6 cm3/mol | ||
| Hazards | |||
| NFPA 704 (fire diamond) |  2 0 0 | ||
| Flash point | Non-flammable | ||
| Related compounds | |||
Other anions | Ammonium fluoride Ammonium chloride Ammonium bromide | ||
Other cations | Sodium iodide Potassium iodide Phosphonium 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  Y N ?) Infobox references | |||
Chemical compound
Ammonium iodide is the inorganic compound with the formula NH4I. A white solid. It is an ionic compound, although impure samples appear yellow. This salt consists of ammonium cation and an iodide anion.[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. Ammonium iodide in aqueous solutions are observed as acidic and display elevated vapor pressures at high temperatures[2]
Preparation
Ammonium iodide can be made in lab by treating ammonia with hydroiodic acid:
- NH3 + HI → NH4I
Uses
Ammonium iodide is used as dietary supplement to treat iodine deficiency.[3]
Properties and Reactions
Ammonium iodide has recently been used in many research studies and experiments.
Vinyl sulfones have been prepared using ammonium iodide,.[4]
Organic reactions are not synthesized with organic solvents due to their increasing detrimental effects on the human body and ecosystem.[5] Many chemists have altered organic reactions to exclude solvents in order to have successful sustainable syntheses. A report was presented on an organic synthesis for the iodination of ketones and aromatic compounds using ammonium iodide and H2O2 (hydrogen peroxide).[5] This resulted in the products' high yields, which were gathered more efficiently, in a shorter duration compared to the use of the abrasive compound: molecular iodine[5]
References
- ^ Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Kirk-Othmer, ed. (2001-01-26). Kirk-Othmer Encyclopedia of Chemical Technology (1 ed.). Wiley. doi:10.1002/0471238961.0113131523051920.a01.pub2. ISBN 978-0-471-48494-3.
- ^ "Ammonium Iodide: Benefits, Risks, and Safety in Dietary Supplements". www.digicomply.com. Retrieved 2023-11-21.
- ^ Gao, Xiaofang; Pan, Xiaojun; Gao, Jian; Huang, Huawen; Yuan, Gaoqing; Li, Yingwei (2015). "Ammonium iodide-induced sulfonylation of alkenes with DMSO and water toward the synthesis of vinyl methyl sulfones". Chemical Communications. 51 (1): 210–212. doi:10.1039/C4CC07606K. PMID 25406694.
- ^ a b c Kulkarni, Pramod; Kondhare, Dasharath; Varala, Ravi; Zubaidha, Pudukulathan (2013). "Cyclization of 2′-hydroxychalcones to flavones using ammonium iodide as an iodine source: An eco-friendly approach". Journal of the Serbian Chemical Society. 78 (7): 909–916. doi:10.2298/jsc120901119k. ISSN 0352-5139.
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Ammonium salts
| monatomic anions |
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| oxyanions |
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| other anions |
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- Aluminon
- Ammonium acetate
- Ammonium adipate
- Ammonium benzoate
- Ammonium bituminosulfonate
- Ammonium carbamate
- Ammonium citrate
- Ammonium diethyl dithiophosphate
- Ammonium ferric citrate
- Ammonium formate
- Ammonium fumarate
- Ammonium glutamate
- Ammonium lactate
- Ammonium lauryl sulfate
- Ammonium malate
- Ammonium nonanoate
- Ammonium oxalate
- Ammonium picrate
- Ammonium perfluorononanoate
- Ammonium propionate
- Ammonium thioglycolate
- Cupferron
- Ferric ammonium oxalate
- Murexide
