|Systematic name||Dioxonitric(III) acid|
|Other names||Nitrous acid|
|Molar mass||47.0134 g/mol|
|Melting point||? °C|
|Boiling point||? °C|
|Disclaimer and references|
Nitrous acid (molecular formula HNO2) is a weak acid known only in solution and in the form of nitrite salts. In the atmosphere, it is formed as an intermediate, breaking down to produce hydroxyl free radicals. These free radicals are then involved in regulating the amount of ozone in the troposphere (lower atmosphere).
Nitrous acid is useful for destroying sodium azide solutions, which are toxic and potentially explosive. It can also be used to prepare diazonium salts, which combine with anilines and phenols to form brightly colored azo compounds. The latter type of reaction can be used to produce azo-dyes, as well as serving as a qualitative test for aromatic amines.
Nitrous acid is readily formed in solution by the action of any mineral acid on sodium nitrite (NaNO2). The reaction may be written as follows:
- NaNO2 + H+ ----> HNO2 + Na+
Nitrous acid is a monobasic acid, which means that each molecule of HNO2 releases one proton (H+) in solution. In addition, it is a weak acid, which means that at any given time, the dissociated molecules are in equilibrium with undissociated molecules.
Also, like other acids, nitrous acid reacts with a base to form a salt. In this case, sodium nitrite is formed.
Nitrous acid is unstable, and it may decompose in two ways, in solution.
- 2HNO2 ----> NO2 + NO + H2O
- 4HNO2 ----> 2HNO3 + N2O + H2O
Nitrous acid is formed in the atmosphere as an important intermediate. It is produced by the reaction of nitrogen dioxide (NO2) and water on various surfaces such as atmospheric aerosols. The action of sunlight then decomposes it to produce hydroxyl free radicals, which are intricately involved in regulating the ozone budget of the troposphere (lower atmosphere).
Nitrous acid is used to destroy toxic and potentially explosive sodium azide solutions. 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.
ReferencesISBN links support NWE through referral fees
- Chang, Raymond. 2006. Chemistry. 9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031
- Cotton, F. Albert, Geoffrey Wilkinson, Carlos A. Murillo, and Manfred Bochmann. 1999. Advanced Inorganic Chemistry. 6th edition. New York: Wiley. ISBN 0471199575
- Greenwood, N.N., and A. Earnshaw. 1998. Chemistry of the Elements. 2nd ed. Oxford, UK; Burlington, MA: Butterworth-Heinemann, Elsevier Science. ISBN 0750633654 Online version Retrieved January 20, 2015.
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