Nitrous acid
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| Nitrous acid | |
|---|---|
 |
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| General | |
| Systematic name | Dioxonitric(III) acid |
| Other names | Nitrous acid |
| Molecular formula | HNO2 |
| Molar mass | 47.0134 g/mol |
| CAS number | 7782-77-6 |
| Properties | |
| Density | ? g/cm3 |
| Solubility (water) | |
| Melting point | ? °C |
| Boiling point | ? °C |
| Acid dissociation constant pKa |
3.34 |
| Disclaimer and references | |
Nitrous acid (molecular formula HNO2) is a weak monobasic acid known only in solution and in the form of nitrite salts.
Nitrous acid is used to make diazides from amines; this occurs by nucleophilic attack of the amine onto the nitrite, reprotonation by the surrounding solvent, and double elimination of water. The diazide can then be liberated as a carbene.
Contents |
[edit] Preparation
It can be prepared by adding any mineral acid to sodium nitrite.
[edit] Decomposition
It rapidly decomposes into nitrogen dioxide, nitric oxide and water when in solution.
2HNO2------>NO2 + NO + H2O
It also decomposes into nitric acid and nitrous oxide and water (?)
4HNO2 -> 2HNO3 + N2O + H2O
[edit] Chemistry
Nitrous acid can be used to prepare diazonium salts which couple with anilines and phenols to form brightly colored azo compounds in a qualitative test for aromatic amines. This reaction is also used to produce azo-dyes. Nitrous acid is used to destroy toxic and potentially explosive sodium azide solutions. Nitrous acid is usually formed in situ by the action of mineral acid on sodium nitrite.
[edit] Atmospheric relevance
Nitrous acid is an important atmospheric intermediate. It is produced by the heterogeneous reaction of NO2 and water on various surfaces such as atmospheric aerosols. It is readily photolysed to produce hydroxyl radicals which are intricately involved in the ozone budget of the troposphere (lower atmosphere).
[edit] See also
[edit] External links
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