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| Names | |
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| IUPAC name
Ammonium nitrite
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| Identifiers | |
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| ChemSpider | |
| ECHA InfoCard | 100.033.257 |
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| [NH4]NO2 | |
| Molar mass | 64.044 g·mol−1 |
| Appearance | colorless or pale yellow crystals |
| Density | 1.69 g/cm3 |
| Melting point | Decomposes |
| 118.3 g / 100mL | |
| Explosive data | |
| Shock sensitivity | Low |
| Friction sensitivity | Low |
| Detonation velocity | >1000 m/s |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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Explosive |
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| Danger | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Non-flammable | |
| Related compounds | |
Other anions
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Ammonium nitrate |
Other cations
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Sodium nitrite |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Ammonium nitrite is a chemical compound with the chemical formula [NH4]NO2. It is the ammonium salt of nitrous acid. It is composed of ammonium cations [NH4]+ and nitrite anions NO−2. It is not used in pure isolated form since it is highly unstable and decomposes into water and nitrogen, even at room temperature.
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Transcription
Preparation
Ammonium nitrite forms naturally in the air and can be prepared by the absorption of equal parts nitrogen dioxide and nitric oxide in aqueous ammonia.[1]
It can also be synthesized by oxidizing ammonia with ozone or hydrogen peroxide, or in a precipitation reaction of barium or lead nitrite with ammonium sulfate, or silver nitrite with ammonium chloride, or ammonium perchlorate with potassium nitrite. The precipitate is filtered off and the solution concentrated. It forms colorless crystals which are soluble in water.
- 2 NH3 + O3 → [NH4]NO2 + H2O
Physical and chemical properties
Ammonium nitrite may explode at a temperature of 60–70 °C,[1] and will decompose quicker when dissolved in a concentrated aqueous solution, than in the form of a dry crystal. Even in room temperature the compound slowly decomposes into water and nitrogen:
- [NH4]NO2 → N2 + 2 H2O
It decomposes when heated or in the presence of acid into water and nitrogen.[2] Ammonium nitrite solution is stable at higher pH and lower temperature. If there is any decrease in pH lower than 7.0, it may lead to an explosion, since the nitrite can react to it. A safe pH can be maintained by adding an ammonia solution. The mole ratio of ammonium nitrite to ammonia must be above 10%.
References
- ^ a b Thomas Scott; Mary Eagleson (1994). Concise encyclopedia chemistry. Walter de Gruyter. p. 66. ISBN 3-11-011451-8.
- ^ "VIAS Encyclopedia: Ammonium Nitrite".
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This page was last edited on 16 May 2024, at 12:11