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Above 330 °C sodium nitrite decomposes (in air) to sodium oxide, nitric oxide and nitrogen dioxide. [88] 2 NaNO 2 → Na 2 O + NO + NO 2. Sodium nitrite can also be used in the production of nitrous acid: 2 NaNO 2 + H 2 SO 4 → 2 HNO 2 + Na 2 SO 4. The nitrous acid then, under normal conditions, decomposes: 2 HNO 2 → NO 2 + NO + H 2 O
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.
Processed meats have no fiber, vitamins, or phytochemical antioxidants, are high in sodium, may contain high fat, and are often fried or cooked at a temperature sufficient to degrade protein into nitrosamines. Nitrates are key intermediates and effectors in the primary vasculature signaling which is necessary for all mammals to survive. [21]
This is a list of CAS numbers by chemical formulas and chemical compounds, ... sodium nitrite: 7632–00–0 NaNO 3: sodium nitrate: 7631–99–4 NaN 3: sodium azide:
A typical procedure entails dissolving sodium nitrite in cold sulfuric acid: [4] [5] HNO 2 + H 2 SO 4 → HSO 4 NO + H 2 O. It can also be prepared by the reaction of nitric acid and sulfur dioxide. [6] HSO 4 NO is used in organic chemistry to prepare diazonium salts from amines, for example in the Sandmeyer reaction.
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