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Copper(II) acetate, also referred to as cupric acetate, is the chemical compound with the formula Cu(OAc) 2 where AcO − is acetate (CH 3 CO − 2).The hydrated derivative, Cu 2 (OAc) 4 (H 2 O) 2, which contains one molecule of water for each copper atom, is available commercially.
The systematic IUPAC name is not always the preferred IUPAC name, for example, lactic acid is a common, and also the preferred, name for what systematic rules call 2-hydroxypropanoic acid. This list is ordered by the number of carbon atoms in a carboxylic acid.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Its chemical formula is usually expressed as Pb(CH 3 COO) 2 or Pb(OAc) 2, where Ac represents the acetyl group. Like many other lead compounds, it causes lead poisoning. Lead acetate is soluble in water and glycerin. With water it forms the trihydrate, Pb(OAc) 2 ·3H 2 O, a colourless or white efflorescent monoclinic crystalline substance.
The acetate anion, [CH 3 COO] −,(or [C 2 H 3 O 2] −) is one of the carboxylate family. It is the conjugate base of acetic acid. Above a pH of 5.5, acetic acid converts to acetate: [1] CH 3 COOH ⇌ CH 3 COO − + H + Many acetate salts are ionic, indicated by their tendency to dissolve well in water.
Copper is a chemical element with the symbol Cu (from Latin: cuprum) and the atomic number of 29. It is easily recognisable, due to its distinct red-orange color.Copper also has a range of different organic and inorganic salts, having varying oxidation states ranging from (0,I) to (III).
The tetrahydrate has been shown by X-ray crystallography to adopt an octahedral structure, the central cobalt centre being coordinated by four water molecules and two acetate ligands. [1] The analogous nickel acetate is isostructural. [2] Various hydrates are known including Co(CH 3 CO 2) 2 ·H 2 O and [Co(CH 3 CO 2) 2] 5 ·0.5 H 2 O. [3]
2 if p CO 2 is less than 0.11 atm. [3] In the presence of water or moist air at 25 °C, CuCO 3 is stable only for p CO 2 above 4.57 atmospheres and pH between about 4 and 8. [8] Below that partial pressure, it reacts with water to form a basic carbonate (azurite, Cu 3 (CO 3) 2 (OH) 2). [3] 3 CuCO 3 + H 2 O → Cu 3 (CO 3) 2 (OH) 2 + CO 2