Hono

Nitrous acid (molecular formula HNO 2 ) is a weak and monoprotic acid known only in solution, in the gas phase and in the form of nitrite (NO− 2 ) salts.[1] Nitrous acid is used to make diazonium salts from amines. The resulting diazonium salts are reagents in azo coupling reactions to give azo dyes.

In the gas phase, the planar nitrous acid molecule can adopt both a syn and an anti form. The anti form predominates at room temperature, and IR measurements indicate it is more stable by around 2.3 kJ/mol.[1]

Dimensions of the anti form (from the microwave spectrum)

Model of the anti form

syn form

Nitrous acid is usually generated by acidification of aqueous solutions of sodium nitrite with a mineral acid. The acidification is usually conducted at ice temperatures, and the HNO2 is consumed in situ.[2][3] Free nitrous acid is unstable and decomposes rapidly.

Nitrous acid can also be produced by dissolving dinitrogen trioxide in water according to the equation

Nitrous acid is the main chemphore in the Liebermann reagent, used to spot-test for alkaloids.

Gaseous nitrous acid, which is rarely encountered, decomposes into nitrogen dioxide, nitric oxide, and water:

Nitrogen dioxide disproportionates into nitric acid and nitrous acid in aqueous solution:[4]

In warm or concentrated solutions, the overall reaction amounts to production of nitric acid, water, and nitric oxide:

The nitric oxide can subsequently be re-oxidized by air to nitric acid, making the overall reaction:

With I− and Fe2+ ions, NO is formed:[5]

With Sn2+ ions, N2O is formed:

With SO2 gas, NH2OH is formed:

With Zn in alkali solution, NH3 is formed:

With N 2 H+ 5 , HN3, and subsequently, N2 gas is formed:

Oxidation by nitrous acid has a kinetic control over thermodynamic control, this is best illustrated that dilute nitrous acid is able to oxidize I− to I2, but dilute nitric acid cannot.

It can be seen that the values of Eo cell for these reactions are similar, but nitric acid is a more powerful oxidizing agent. Base on the fact that dilute nitrous acid can oxidize iodide into iodine, it can be deduced that nitrous is a faster, rather than a more powerful, oxidizing agent than dilute nitric acid.[5]

Nitrous acid is used to prepare diazonium salts:

where Ar is an aryl group.

Such salts are widely used in organic synthesis, e.g., for the Sandmeyer reaction and in the preparation azo dyes, brightly colored compounds that are the basis of a qualitative test for anilines.[6] Nitrous acid is used to destroy toxic and potentially explosive sodium azide. For most purposes, nitrous acid is usually formed in situ by the action of mineral acid on sodium nitrite:[7] It is mainly blue in colour

Reaction with two α-hydrogen atoms in ketones creates oximes, which may be further oxidized to a carboxylic acid, or reduced to form amines. This process is used in the commercial production of adipic acid.

Nitrous acid reacts rapidly with aliphatic alcohols to produce alkyl nitrites, which are potent vasodilators:

The carcinogens called nitrosamines are produced, usually not intentionally, by the reaction of nitrous acid with secondary amines:

Nitrous acid is involved in the ozone budget of the lower atmosphere, the troposphere. The heterogeneous reaction of nitric oxide (NO) and water produces nitrous acid. When this reaction takes place on the surface of atmospheric aerosols, the product readily photolyses to hydroxyl radicals.[8][9]