Experimental Solubility: 119% w/w in 0?C water Kaye & Laby (No longer updated)ġ70% w/w in 100?C water Kaye & Laby (No longer updated).Experimental Boiling Point: 120 ☌ (Decomposes) OU Chemical Safety Data (No longer updated) More details.Experimental Physico-chemical Properties.
Sodium acetate molar mass skin#
This salt is mildly irritating of eyes, skin and respiratory tract. It is incompatible with strong oxidizing agents. Health effects/safety hazards: Sodium acetate is stable. Moreover, sodium acetate is used in neutralizationof sulfuric acid waste in the textile industry. Sodium acetate solution is used as medicine alternative to sodium chloride to provide sodium ion (Na +) to the organism.Īs mentioned in the chemical properties, sodium acetate is used to buffering solutions, especially to biochemical and pharmaceutical application.
For example, in the fries potatoes chips, it is used as a salt and vinegar flavor. In food industries, sodium acetate is added as a seasoning due its vinegar taste. Uses: Sodium acetate is widely use by the food, pharmaceutical and chemical industries. When heat is above 324 ✬, this salt decomposes, producing acetic acid fumes. Sodium acetate solution in water is weak alkaline. Sodium acetate is higly soluble in water (the solubility is 46.5 g sodium acetate in 100 mL of water).Ĭhemical properties: Sodium acetate is the conjugated base of acetic acid, thus a solution of acetic acid/sodium acetate can be used to prepare buffer solutions, in order to control pH. Physical properties: Sodium acetate is a hygroscopic white crystalline powder with vinager (acetic acid) odor. If the reaction is prepared with sodium hydroxide, sodium acetate and water will be the only products.
Carbonic acid readily decomposes under normal conditions into carbon dioxide and water. When the reaction includes sodium carbonate or bicarbonates, it produces carbonic acid and sodium acetate. The synthesis uses vinegar (acetic acid 5-8%) or glacial acetic acid, washing soda (sodium carbonate) or baking soda (sodium bicarbonate) or sodium hydroxide. Preparation: Sodium acetate can be prepared through a very simple and cheap reaction consisting in the neutralization of acetic acid. Both of the ion, Na + and CH 3COO - are present in the organisms and exerting vital roles: sodium ion as regulator of total body water and acetate ion as hydrogen acceptor. This salt can be found in either, the anhydrous or trihydrated form. Occurrence: Sodium acetate occurs naturally in plants and animals tissues. Its chemical structure can be written as below, in the common representations used for organic molecules. Its molecular formula is C 2H 3NaO 2 and its molar mass is 82.03 g mol -1. Formula and structure: The chemical formula of sodium acetate is CH 3COONa.
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