|Jmol-3D images||Image 1|
|Molar mass||64.06 g/mol|
|Appearance||pale yellow crystals, slowly decomposes to nitrogen and water|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
It can also be prepared 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 and decompose on heating or in the presence of acid, with the formation of nitrogen. 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 explosion. It is desirable to maintain pH by adding ammonia solution. The mole ratio of Ammonium Nitrite to Ammonia must be above 10% mole ratio.
- NH4NO2 → N2 + 2 H2O
Ammonium nitrite may explode at a temperature of 60–70 °C. It decomposes more quickly when a concentrated solution than when it is a dry crystal.
- "Ammonium nitrite - Identification, toxicity, use, water pollution potential, ecological toxicity and regulatory information". PAN Pesticides Database - Chemicals. Retrieved 2006-07-26.
- 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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