Nitrous acid

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. Image:Trans-nitrous-acid-2D-dimensions.png | Dimensions of the anti form(from the microwave spectrum) Image:Trans-nitrous-acid-3D-balls.png | Model of the anti form Image:Cis-nitrous-acid-3D-balls.png | syn form ==Decomposition and preparation==

Free, gaseous nitrous acid is unstable, rapidly disproportionating to nitric oxides: :2 HNO2 → NO2 + NO + H2O In aqueous solution, the nitrogen dioxide also disproportionates, for a net reaction producing nitric oxide and nitric acid: :3 HNO2 → 2 NO + HNO3 + Consequently applications of nitrous acid usually begin with mineral acid acidification of sodium nitrite. The acidification is usually conducted at ice temperatures, and the HNO2 consumed in situ. Nitrous acid equilibrates with dinitrogen trioxide in water, so that concentrated solutions are visibly blue: : N2O3 + H2O 2 HNO2 Addition of dinitrogen trioxide to water is thus another preparatory technique. ==Chemical applications==

Nitrous acid is the main chemophore in the Liebermann reagent, used to spot-test for alkaloids. At high acidities (), nitrous acid is protonated to give water and nitrosonium cations. : 2 HNO2 + 2 KI + 2 H2SO4 → I2 + 2 NO + 2 H2O + 2 K2SO4 : 2 HNO2 + 2 FeSO4 + 2 H2SO4 → Fe2(SO4)3 + 2 NO + 2 H2O + K2SO4 With Sn2+ ions, N2O is formed: : 2 HNO2 + 4 HCl + 2 SnCl2 → 2 SnCl4 + N2O + 3 H2O With SO2 gas, NH2OH is formed: : 2 KNO2 + 6 H2O + 4 SO2 → 3 H2SO4 + K2SO4 + 2 NH2OH With Zn in alkali solution, NH3 is formed: : 5 H2O + KNO2 + 3 Zn → NH3 + KOH + 3 Zn(OH)2 With , both HN3 and (subsequently) N2 gas are formed: : HNO2 + [N2H5]+ → HN3 + H2O + H3O+ : HNO2 + HN3 → N2O + N2 + H2O 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. : I2 + 2 e− ⇌ 2 I− Eo = +0.54 V : + 3 H+ + 2 e− ⇌ HNO2 + H2O Eo = +0.93 V : HNO2 + H+ + e− ⇌ NO + H2O Eo = +0.98 V It can be seen that the values of E for these reactions are similar, but nitric acid is a more powerful oxidizing agent. Based 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. 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: It is mainly blue in colour : NaNO2 + HCl → HNO2 + NaCl : 2 NaN3 + 2 HNO2 → 3 N2 + 2 NO + 2 NaOH 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: :(CH3)2CHCH2CH2OH + HNO2 → (CH3)2CHCH2CH2ONO + H2O The carcinogens called nitrosamines are produced, usually not intentionally, by the reaction of nitrous acid with secondary amines: :HNO2 + R2NH → R2N-NO + H2O ==Atmosphere of the Earth==

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. ==DNA damage and mutation==

Treatment of Escherichia coli cells with nitrous acid causes damage to the cell's DNA including deamination of cytosine to uracil, and these damages are subject to repair by specific enzymes. Also, nitrous acid causes base substitution mutations in organisms with double-stranded DNA. ==See also==