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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 .
In the NO − 3 anion, the oxidation state of the central nitrogen atom is V (+5). This corresponds to the highest possible oxidation number of nitrogen. Nitrate is a potentially powerful oxidizer as evidenced by its explosive behaviour at high temperature when it is detonated in ammonium nitrate (NH 4 NO 3), or black powder, ignited by the shock wave of a primary explosive.
The nitrate anion is an oxidizer, and many tests for the nitrate anion are based on this property. However, other oxidants present in the analyte may interfere and give erroneous results. Nitrate can also be detected by first reducing it to the more reactive nitrite ion and using one of many nitrite tests. [1]
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.
Typically, denitrification occurs in anoxic environments, where the concentration of dissolved and freely available oxygen is depleted. In these areas, nitrate (NO 3 −) or nitrite (NO 2 −) can be used as a substitute terminal electron acceptor instead of oxygen (O 2), a more energetically favourable electron acceptor. Terminal electron ...
Ammonium nitrate is a chemical compound with the formula NH 4 NO 3. It is a white crystalline salt consisting of ions of ammonium and nitrate. It is highly soluble in water and hygroscopic as a solid, but does not form hydrates. It is predominantly used in agriculture as a high-nitrogen fertilizer. [5]
In the solid state it is ionic with structure [NO 2] + [NO 3] −; as a gas and in solution it is molecular O 2 N–O–NO 2. Hydration to nitric acid comes readily, as does analogous reaction with hydrogen peroxide giving peroxonitric acid (HOONO 2). It is a violent oxidising agent. Gaseous dinitrogen pentoxide decomposes as follows: [15]
Ingesting too much nitrite and/or nitrate through well water is suspected to cause methemoglobinemia. [19] 95% of the nitrite ingested in modern diets comes from bacterial conversion of nitrates naturally found in vegetables. [20] However, potentially cancer-causing nitroso compounds are not made in the pH-neutral colon.