[{"@context":"http:\/\/schema.org\/","@type":"BlogPosting","@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/cobaltii-sulfate-wikipedia\/#BlogPosting","mainEntityOfPage":"https:\/\/wiki.edu.vn\/en\/wiki40\/cobaltii-sulfate-wikipedia\/","headline":"Cobalt(II) sulfate – Wikipedia","name":"Cobalt(II) sulfate – Wikipedia","description":"From Wikipedia, the free encyclopedia Inorganic compound Cobalt(II) sulfate Names IUPAC name Cobalt(II) sulfate Other names Cobaltous sulfate Identifiers ChEBI","datePublished":"2019-09-08","dateModified":"2019-09-08","author":{"@type":"Person","@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/author\/lordneo\/#Person","name":"lordneo","url":"https:\/\/wiki.edu.vn\/en\/wiki40\/author\/lordneo\/","image":{"@type":"ImageObject","@id":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","url":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","height":96,"width":96}},"publisher":{"@type":"Organization","name":"Enzyklop\u00e4die","logo":{"@type":"ImageObject","@id":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","url":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","width":600,"height":60}},"image":{"@type":"ImageObject","@id":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/4\/41\/Cobaltsulfat.JPG\/220px-Cobaltsulfat.JPG","url":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/4\/41\/Cobaltsulfat.JPG\/220px-Cobaltsulfat.JPG","height":"220","width":"220"},"url":"https:\/\/wiki.edu.vn\/en\/wiki40\/cobaltii-sulfate-wikipedia\/","wordCount":5353,"articleBody":"From Wikipedia, the free encyclopediaInorganic compoundCobalt(II) sulfateNamesIUPAC nameCobalt(II) sulfateOther namesCobaltous sulfateIdentifiersChEBIChemSpiderECHA InfoCard100.030.291 EC NumberKEGGRTECS numberGG3100000 (anhydrous) GG3200000 (heptahydrate)UNIIInChI=1S\/Co.H2O4S\/c;1-5(2,3)4\/h;(H2,1,2,3,4)\/q+2;\/p-2\u00a0YKey:\u00a0KTVIXTQDYHMGHF-UHFFFAOYSA-L\u00a0YInChI=1\/Co.H2O4S\/c;1-5(2,3)4\/h;(H2,1,2,3,4)\/q+2;\/p-2Key:\u00a0KTVIXTQDYHMGHF-NUQVWONBAJPropertiesCoSO4\u00b7(H2O)n (n=0,1,6,7)Molar mass154.996 g\/mol (anhydrous) 173.01 g\/mol (monohydrate) 263.08 g\/mol (hexahydrate) 281.103 g\/mol (heptahydrate)Appearancereddish crystalline (anhydrous, monohydrate) pink salt (hexahydrate)Odorodorless (heptahydrate)Density3.71 g\/cm3 (anhydrous) 3.075 g\/cm3 (monohydrate) 2.019 g\/cm3 (hexahydrate) 1.948 g\/cm3 (heptahydrate)Melting point735\u00a0\u00b0C (1,355\u00a0\u00b0F; 1,008\u00a0K)anhydrous: 36.2 g\/100 mL (20\u00a0\u00b0C) 38.3 g\/100 mL (25 \u00b0C) 84 g\/100 mL (100 \u00b0C) heptahydrate: 60.4 g\/100 mL (3 \u00b0C) 67 g\/100 mL (70 \u00b0C)Solubilityanhydrous: 1.04 g\/100 mL (methanol, 18 \u00b0C) insoluble in ammonia heptahydrate: 54.5 g\/100 mL (methanol, 18 \u00b0C)+10,000\u00b710\u22126 cm3\/mol1.639 (monohydrate) 1.540 (hexahydrate) 1.483 (heptahydrate)Structureorthorhombic (anhydrous) monoclinic (monohydrate, heptahydrate)HazardsGHS labelling:DangerH302, H317, H334, H341, H350, H360, H410P201, P202, P261, P264, P270, P272, P273, P280, P281, P285, P301+P312, P302+P352, P304+P341, P308+P313, P321, P330, P333+P313, P342+P311, P363, P391, P405, P501NFPA 704 (fire\u00a0diamond)Flash pointNon-flammableLethal dose or concentration (LD, LC):424 mg\/kg (oral, rat)Safety data sheet (SDS)JT Baker MSDSExcept where otherwise noted, data are given for materials in their standard state (at 25\u00a0\u00b0C [77\u00a0\u00b0F], 100\u00a0kPa).Chemical compound  Cobalt(II) sulfate heptahydrateCobalt(II) sulfate is any of the inorganic compounds with the formula CoSO4(H2O)x.  Usually cobalt sulfate refers to the hexa- or heptahydrates CoSO4.6H2O or CoSO4.7H2O, respectively.[1] The heptahydrate is a red solid that is soluble in water and methanol. Since cobalt(II) has an odd number of electrons, its salts are paramagnetic.Table of ContentsPreparation, and structure[edit]Uses and reactions[edit]Natural occurrence[edit]Health issues[edit]Related compounds[edit]References[edit]Preparation, and structure[edit]It forms by the reaction of metallic cobalt, its oxide, hydroxide, or carbonate with aqueous sulfuric acid:[1]Co  +  H2SO4  +  7 H2O  \u2192  CoSO4(H2O)7  +  H2CoO  +  H2SO4  +  6 H2O  \u2192  CoSO4(H2O)7The heptahydrate is only stable at humidity >70% at room temperature, otherwise it converts to the hexahydrate.[2]  The hexahydrate converts to the monohydrate and the anhydrous forms at 100 and 250\u00a0\u00b0C, respectively.[1]CoSO4(H2O)7  \u2192 CoSO4(H2O)6 +  H2OCoSO4(H2O)6  \u2192 CoSO4(H2O) +  5\u00a0H2OCoSO4(H2O)  \u2192 CoSO4 +  H2OThe hexahydrate is a metal aquo complex consisting of octahedral [Co(H2O)6]2+ ions associated with sulfate anions (see image in table).[3] The monoclinic heptahydrate has also been characterized by X-ray crystallography. It also features [Co(H2O)6]2+ octahedra as well as one water of crystallization.[2]Uses and reactions[edit]Cobalt sulfates are important intermediates in the extraction of cobalt from its ores.  Thus, crushed, partially refined ores are treated with sulfuric acid to give red-colored solutions containing cobalt sulfate.[1]Hydrated cobalt(II) sulfate is used in the preparation of pigments, as well as in the manufacture of other cobalt salts. Cobalt pigment is used in porcelains and glass. Cobalt(II) sulfate is used in storage batteries and electroplating baths, sympathetic inks, and as an additive to soils and animal feeds.  For these purposes, the cobalt sulfate is produced by treating cobalt oxide with sulfuric acid.[1]Being commonly available commercially, the heptahydrate is a routine source of cobalt in coordination chemistry.[4]Natural occurrence[edit]Rarely, cobalt(II) sulfate is found in form of few crystallohydrate minerals, occurring among oxidation zones containing primary Co minerals (like skutterudite or cobaltite). These minerals are: biebierite (heptahydrate), moorhouseite (Co,Ni,Mn)SO4.6H2O,[5][6] aplowite (Co,Mn,Ni)SO4.4H2O and cobaltkieserite (monohydrate).[7][8][6]Health issues[edit]Cobalt is an essential mineral for mammals, but more than a few micrograms per day is harmful.  Although poisonings have rarely resulted from cobalt compounds, their chronic ingestion has caused serious health problems at doses far less than the lethal dose. In 1965, the addition of a cobalt compound to stabilize beer foam in Canada led to a peculiar form of toxin-induced cardiomyopathy, which came to be known as beer drinker’s cardiomyopathy.[9][10][11]Furthermore, cobalt(II) sulfate is suspected of causing cancer (i.e., possibly carcinogenic, IARC Group 2B) as per the International Agency for Research on Cancer (IARC) Monographs.[12]Related compounds[edit]References[edit]^ a b c d e Donaldson, John Dallas; Beyersmann, Detmar (2005). “Cobalt and Cobalt Compounds”. Ullmann’s Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002\/14356007.a07_281.pub2.^ a b Redhammer, G. J.; Koll, L.; Bernroider, M.; Tippelt, G.; Amthauer, G.; Roth, G. (2007). “Co2+-Cu2+ Substitution in Bieberite Solid-Solution Series, (Co1\u2212xCux)SO4 \u00b7 7H2O, 0.00 \u2264 x \u2264 0.46: Synthesis, Single-Crystal Structure Analysis, and Optical Spectroscopy”. American Mineralogist. 92 (4): 532\u2013545. Bibcode:2007AmMin..92..532R. doi:10.2138\/am.2007.2229. S2CID\u00a095885758.^ Elerman, Y. “Refinement of the Crystal Structure of CoSO4 \u00b7 6H2O” Acta Crystallographica Section C 1988, volume 44, p599-p601. doi:10.1107\/S0108270187012447^ Broomhead, J. A.; Dwyer, F. P.; Hogarth, J. W. (1950). Resolution of the Tris(ethylenediamine)cobalt(III) Ion. Inorganic Syntheses. Vol.\u00a06. pp.\u00a0183\u2013186. doi:10.1002\/9780470132371.ch58. ISBN\u00a09780470132371.^ “Moorhouseite”.^ a b “List of Minerals”. 21 March 2011.^ “Cobaltkieserite”.^ “Bieberite”.^ Morin Y; T\u011btu A; Mercier G (1969). “Quebec beer-drinkers’ cardiomyopathy: Clinical and hemodynamic aspects”. Annals of the New York Academy of Sciences. 156 (1): 566\u2013576. Bibcode:1969NYASA.156..566M. doi:10.1111\/j.1749-6632.1969.tb16751.x. PMID\u00a05291148. S2CID\u00a07422045.^ Barceloux, Donald G. & Barceloux, Donald (1999). “Cobalt”. Clinical Toxicology. 37 (2): 201\u2013216. doi:10.1081\/CLT-100102420. PMID\u00a010382556.^ 11.1.5 The unusual type of myocardiopathy recognized in 1965 and 1966 in Quebec (Canada), Minneapolis (Minnesota), Leuven (Belgium), and Omaha (Nebraska) was associated with episodes of acute heart failure (e\/g\/, 50 deaths among 112 beer drinkers).^ “Cobalt in Hard Metals and Cobalt Sulfate, Gallium Arsenide, Indium Phosphide and Vanadium Pentoxide” (PDF). IARC Monographs on the Evaluation of Carcinogenic Risks to Humans.Compounds containing the sulfate group (SO2\u22124)"},{"@context":"http:\/\/schema.org\/","@type":"BreadcrumbList","itemListElement":[{"@type":"ListItem","position":1,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/#breadcrumbitem","name":"Enzyklop\u00e4die"}},{"@type":"ListItem","position":2,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki40\/cobaltii-sulfate-wikipedia\/#breadcrumbitem","name":"Cobalt(II) sulfate – Wikipedia"}}]}]