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The nitrite ion has the chemical formula NO − 2. Nitrite (mostly sodium nitrite) is widely used throughout chemical and pharmaceutical industries. [1] The nitrite anion is a pervasive intermediate in the nitrogen cycle in nature. The name nitrite also refers to organic compounds having the –ONO group, which are esters of nitrous acid.
Nitrite is a precursor to carcinogenic nitrosamines, and; via the formation of nitrite, nitrate is implicated in methemoglobinemia, a disorder of hemoglobin in red blood cells susceptible to especially affect infants and toddlers. [11] [12]
A nitrate nitrite, or nitrite nitrate, is a coordination complex or other chemical compound that contains both nitrite (NO − 2) and nitrate (NO − 3) anions. They are mixed-anion compounds, and they are mixed-valence compounds. Some have third anions. Many nitrite nitrate compounds are coordination complexes of cobalt.
Sodium nitrite is an inorganic compound with the chemical formula Na N O 2. It is a white to slightly yellowish crystalline powder that is very soluble in water and is hygroscopic . From an industrial perspective, it is the most important nitrite salt.
Nitrogen cycle. Nitrification is the biological oxidation of ammonia to nitrate via the intermediary nitrite.Nitrification is an important step in the nitrogen cycle in soil.The process of complete nitrification may occur through separate organisms [1] or entirely within one organism, as in comammox bacteria.
The Griess test is an analytical chemistry test which detects the presence of nitrite ion in solution. One of its most important uses is the determination of nitrite in drinking water. The Griess diazotization reaction, on which the Griess reagent relies, was first described in 1858 by Peter Griess.
Nitromethane can be produced in the laboratory by treating sodium chloroacetate with sodium nitrite. [7] Oxidation of oximes [8] or primary amines. [9] Reduction of β-nitro alcohols [10] or nitroalkenes. [11] By decarboxylation of α-nitro carboxylic acids formed from nitriles and ethyl nitrate. [12] [13]
Ammonium nitrite forms naturally in the air and can be prepared by the absorption of equal parts nitrogen dioxide and nitric oxide in aqueous ammonia. [1]It can also be synthesized by oxidizing ammonia with ozone or hydrogen peroxide, or in a precipitation reaction of barium or lead nitrite with ammonium sulfate, or silver nitrite with ammonium chloride, or ammonium perchlorate with potassium ...