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3 NO 2 + H 2 O → 2 HNO 3 + NO. The net reaction is maximal oxidation of ammonia: NH 3 + 2 O 2 → HNO 3 + H 2 O. Dissolved nitrogen oxides are either stripped (in the case of white fuming nitric acid) or remain in solution to form red fuming nitric acid. Commercial grade nitric acid solutions are usually between 52% and 68% nitric acid by ...
It is a multi-step nitrogen fixation reaction that uses electrical arcs to react atmospheric nitrogen (N 2) with oxygen (O 2), ultimately producing nitric acid (HNO 3) with water. [1] The resultant nitric acid was then used as a source of nitrate (NO 3 −) in the reaction + + + which may take place in the presence of water or another proton ...
Solutions of dinitrogen pentoxide in nitric acid can be seen as nitric acid with more than 100% concentration. The phase diagram of the system H 2 O − N 2 O 5 shows the well-known negative azeotrope at 60% N 2 O 5 (that is, 70% HNO 3 ), a positive azeotrope at 85.7% N 2 O 5 (100% HNO 3 ), and another negative one at 87.5% N 2 O 5 ("102% HNO 3 ").
2 HNO 3 ⇌ H 2 NO + 3 + NO − 3 ⇌ H 2 O + [NO 2] + + [NO 3] −. Two hydrates, HNO 3 ·H 2 O and HNO 3 ·3H 2 O, are known that can be crystallised. It is a strong acid and concentrated solutions are strong oxidising agents, though gold, platinum, rhodium, and iridium are immune to attack.
A number of side reactions compete with the formation of nitric oxide. Some reactions convert the ammonia to N 2, such as: 4NH 3 + 6NO → 5N 2 + 6H 2 O. This is a secondary reaction that is minimised by reducing the time the gas mixtures are in contact with the catalyst. [6] Another side reaction produces nitrous oxide:
Indeed silver nitrate can be prepared by dissolving silver in nitric acid followed by evaporation of the solution. The stoichiometry of the reaction depends upon the concentration of nitric acid used. 3 Ag + 4 HNO 3 (cold and diluted) → 3 AgNO 3 + 2 H 2 O + NO Ag + 2 HNO 3 (hot and concentrated) → AgNO 3 + H 2 O + NO 2
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 +).
At night, NO 3 further reacts with NO 2 and establishes an equilibrium reaction with dinitrogen pentoxide (N 2 O 5). [36] Via heterogeneous reaction, N 2 O 5 reacts with water vapor or liquid water and forms nitric acid (HNO 3). As mentioned above, nitric acid can be removed through wet and dry deposition and this results in the removal of NO x ...