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Nitric acid is an inorganic compound with the formula H N O 3.It is a highly corrosive mineral acid. [6] The compound is colorless, but samples tend to acquire a yellow cast over time due to decomposition into oxides of nitrogen.
In the United States of America, over seven million tonnes of nitric acid are produced every year, most of which is used for nitrate production for fertilisers and explosives, among other uses. Anhydrous nitric acid may be made by distilling concentrated nitric acid with phosphorus pentoxide at low pressure in glass apparatus in the dark.
Acid strength is the tendency of an acid, symbolised by the chemical formula , to dissociate ... , nitric acid () and sulfuric acid (). A weak acid is ...
The Ostwald process begins with burning ammonia.Ammonia burns in oxygen at temperature about 900 °C (1,650 °F) and pressure up to 8 standard atmospheres (810 kPa) [4] in the presence of a catalyst such as platinum gauze, alloyed with 10% rhodium to increase its strength and nitric oxide yield, platinum metal on fused silica wool, copper or nickel to form nitric oxide (nitrogen(II) oxide) and ...
Nitric acid (HNO 3) is an acid because it donates a proton to the water molecule and its conjugate base is nitrate (NO − 3). The water molecule acts as a base because it receives the hydrogen cation (proton) and its conjugate acid is the hydronium ion (H 3 O +).
Mixture of nitric and acetic acids or nitric acid and acetic anhydride is commercially important in the production of RDX, as amines are destructed by sulfuric acid. Acetyl nitrate had also been used as a nitration agent. [14] [15] In the Wolffenstein–Böters reaction, benzene reacts with nitric acid and mercury(II) nitrate to give picric acid.
Nitrous acid (molecular formula H N O 2) is a weak and monoprotic acid known only in solution, in the gas phase, and in the form of nitrite (NO − 2) salts. [3] It was discovered by Carl Wilhelm Scheele, who called it "phlogisticated acid of niter".
These are thought to be the principal pathways for formation of nitric acid in the atmosphere. [8]: 224–225 This nitric acid contributes to acid rain or may deposit to soil, where it makes nitrate, which is of use to growing plants. The aqueous phase reaction 2 NO 2 + H 2 O → HNO 2 + HNO 3
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