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Copper(II) sulfate is an inorganic compound with the chemical formula Cu SO 4.It forms hydrates CuSO 4 ·nH 2 O, where n can range from 1 to 7. The pentahydrate (n = 5), a bright blue crystal, is the most commonly encountered hydrate of copper(II) sulfate, [10] while its anhydrous form is white. [11]
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 oxidation state of oxygen is −2 in almost all known compounds of oxygen. The oxidation state −1 is found in a few compounds such as peroxides . Compounds containing oxygen in other oxidation states are very uncommon: − 1 ⁄ 2 ( superoxides ), − 1 ⁄ 3 ( ozonides ), 0 (elemental, hypofluorous acid ), + 1 ⁄ 2 ( dioxygenyl ), +1 ...
The +2 oxidation state copper (or other metal in the isomorphic series) is in a distorted octahedral coordination surrounded by four oxygen atoms and two water molecules. [ 7 ] The X-ray photoelectron spectrum of Chevreul's salt shows peaks at 955.6, 935.8, 953.3 and 943.9 eV that correspond to Cu(II) 2 p 1/2 , 2 p 3/2 , Cu(I) 2 p 1/2 , 2 p 3/2 .
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.
Iron(II) sulfate outside a titanium dioxide factory in Kaanaa, Pori, Finland. Upon dissolving in water, ferrous sulfates form the metal aquo complex [Fe(H 2 O) 6] 2+, which is an almost colorless, paramagnetic ion. On heating, iron(II) sulfate first loses its water of crystallization and the original green crystals are converted into a white ...
The ores are treated with an aqueous mixture of ammonium carbonate, ammonia, and oxygen to ultimately give copper(II) ammine complex carbonates, such as [Cu(NH 3) 4]CO 3. After extraction from the residues and after separation from iron, lead, etc. impurities, the carbonate salt is decomposed with steam to give CuO. [3]
Cu 2 S reacts with oxygen to form SO 2: [6] 2 Cu 2 S + 3 O 2 → 2 Cu 2 O + 2 SO 2. The production of copper from chalcocite is a typical process in extracting the metal from ores. Usually, the conversion involves roasting, to give Cu 2 O and sulfur dioxide: [6] Cu 2 S + O 2 → 2 Cu + SO 2. Cuprous oxide readily converts to copper metal upon ...