Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Cobalt(II) sulfate: Difference between pages

{{Short description|Inorganic compound}}

| Verifiedfields = changed

| verifiedrevid = 476995619

| ImageFile1 = Cobaltsulfat.JPG

| ImageSize = 260 px

| ImageName = Cobalt(II) sulfate hydrate

| ImageFile2 = Coaq6SO4.tif

| ImageSize2 =

| ImageName2 = Cobalt(II) sulfate Xray

| OtherNames = Cobaltous sulfate

|Section1={{Chembox Identifiers

| UNII3_Ref = {{fdacite|correct|FDA}}

| UNII3 = Y8N698ZE0T

| UNII3_Comment = (heptahydrate)

| CASNo = 10124-43-3

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo2_Ref = {{cascite|correct|CAS}}

| CASNo2 = 13455-34-0

| CASNo2_Comment = (monohydrate)

| CASNo3_Ref = {{cascite|correct|CAS}}

| CASNo3 = 10026-24-1

| CASNo3_Comment = (heptahydrate)

| KEGG = C17383

| KEGG3 = C19215

| KEGG3_Comment = (heptahydrate)

}}

|Section2={{Chembox Properties

| Formula = CoSO₄·(H₂O)_n (n=0,1,6,7)

| MolarMass = 154.996 g/mol (anhydrous) <br> 173.01 g/mol (monohydrate) <br> 263.08 g/mol (hexahydrate) <br> 281.103 g/mol (heptahydrate)

| Appearance = reddish crystalline (anhydrous, monohydrate) <br> pink salt (hexahydrate)

| Odor = odorless (heptahydrate)

| Density = 3.71 g/cm³ (anhydrous) <br> 3.075 g/cm³ (monohydrate) <br> 2.019 g/cm³ (hexahydrate) <br> 1.948 g/cm³ (heptahydrate)

| Solubility = ''anhydrous:'' <br> 36.2 g/100 mL (20&nbsp;°C) <br> 38.3 g/100 mL (25 °C) <br> 84 g/100 mL (100 °C) <hr> ''heptahydrate:'' <br> 60.4 g/100 mL (3 °C) <br> 67 g/100 mL (70 °C)

| SolubleOther = ''anhydrous:'' <br> 1.04 g/100 mL (methanol, 18 °C) <br> insoluble in [[ammonia]] <hr> ''heptahydrate:'' <br> 54.5 g/100 mL (methanol, 18 °C)

| MeltingPtC = 735

| MeltingPt_notes =

| BoilingPtC =

| BoilingPt_notes =

| RefractIndex = 1.639 (monohydrate) <br> 1.540 (hexahydrate) <br> 1.483 (heptahydrate)

| MagSus = +10,000·10⁻⁶ cm³/mol}}

|Section3={{Chembox Structure

| CrystalStruct = orthorhombic (anhydrous) <br> monoclinic (monohydrate, heptahydrate)}}

|Section7={{Chembox Hazards

| ExternalSDS = [https://www.inchem.org/documents/icsc/icsc/eics1396.htm ICSC 1396] (heptahydrate)

| GHSPictograms = {{GHS07}}{{GHS08}}{{GHS09}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|302|317|334|341|350|360|410}}

| PPhrases = {{P-phrases|201|202|261|264|270|272|273|280|281|285|301+312|302+352|304+341|308+313|321|330|333+313|342+311|363|391|405|501}}

| NFPA-S =

| PEL = }}}}

[[File:Сульфат кобальта гептагидрат.jpg|alt=Cobalt(II) sulfate|thumb|Cobalt(II) sulfate heptahydrate]]

'''Cobalt(II) sulfate''' is any of the [[inorganic compound]]s with the formula CoSO₄(H₂O)_x. Usually cobalt sulfate refers to the hexa- or heptahydrates CoSO₄^.6H₂O or CoSO₄^.7H₂O, respectively.<ref name=Ullmann/> 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]].

==Preparation, and structure==

It forms by the reaction of metallic cobalt, its oxide, hydroxide, or carbonate with aqueous sulfuric acid:<ref name=Ullmann/>

:{{chem2 | Co + H2SO4 + 7 H2O -> CoSO4(H2O)7 + H2 }}

:{{chem2 | CoO + H2SO4 + 6 H2O -> CoSO4(H2O)7 }}

The heptahydrate is only stable at humidity >70% at room temperature, otherwise it converts to the hexahydrate.<ref name=Redhammer/> The hexahydrate converts to the monohydrate and the anhydrous forms at 100 and 250&nbsp;°C, respectively.<ref name=Ullmann/>

:{{chem2 | CoSO4(H2O)7 -> CoSO4(H2O)6 + H2O }}

:{{chem2 | CoSO4(H2O)6 -> CoSO4(H2O) + 5 H2O }}

:{{chem2 | CoSO4(H2O) -> CoSO4 + H2O }}

The hexahydrate is a [[metal aquo complex]] consisting of [[octahedral molecular geometry|octahedral]] [Co(H₂O)₆]²⁺ ions associated with [[sulfate]] [[anions]] (see image in table).<ref>{{cite journal | doi = 10.1107/S0108270187012447| title = Refinement of the crystal structure of CoSO4.6H2O| date = 1988| last1 = Elerman| first1 = Y.| journal = Acta Crystallographica Section C Crystal Structure Communications| volume = 44| issue = 4| pages = 599–601| bibcode = 1988AcCrC..44..599E}}</ref> 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]].<ref name=Redhammer>{{cite journal |doi=10.2138/am.2007.2229|title=Co²⁺-Cu²⁺ Substitution in Bieberite Solid-Solution Series, (Co_1−x''Cu_x'')SO₄ · 7H₂O, 0.00 ≤ x ≤ 0.46: Synthesis, Single-Crystal Structure Analysis, and Optical Spectroscopy|year=2007|last1=Redhammer|first1=G. J.|last2=Koll|first2=L.|last3=Bernroider|first3=M.|last4=Tippelt|first4=G.|last5=Amthauer|first5=G.|last6=Roth|first6=G.|journal=American Mineralogist|volume=92|issue=4|pages=532–545|bibcode=2007AmMin..92..532R|s2cid=95885758}}</ref>

==Uses and reactions==

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.<ref name=Ullmann>{{Ullmann|doi=10.1002/14356007.a07_281.pub2|title=Cobalt and Cobalt Compounds|year=2005|last1=Donaldson|first1=John Dallas|last2=Beyersmann|first2=Detmar|isbn=3527306730}}</ref>

Hydrated cobalt(II) sulfate is used in the preparation of [[pigment]]s, 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 [[Battery (electricity)|batteries]] and [[electroplating]] baths, [[sympathetic ink]]s, and as an additive to soils and animal feeds. For these purposes, the cobalt sulfate is produced by treating cobalt oxide with sulfuric acid.<ref name=Ullmann/>

Being commonly available commercially, the heptahydrate is a routine source of cobalt in [[coordination chemistry]].<ref>{{cite book |doi=10.1002/9780470132371.ch58|title=Inorganic Syntheses|year=1950|volume=6|last1=Broomhead|first1=J. A.|last2=Dwyer|first2=F. P.|last3=Hogarth|first3=J. W.|chapter=Resolution of the Tris(ethylenediamine)cobalt(III) Ion |pages=183–186|isbn=9780470132371}}</ref>

==Natural occurrence==

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,<ref>{{Cite web|url=https://www.mindat.org/min-2776.html|title=Moorhouseite}}</ref><ref name="ima-mineralogy.org"/> aplowite (Co,Mn,Ni)SO₄^.4H₂O and cobaltkieserite (monohydrate).<ref>{{Cite web|url=https://www.mindat.org/min-26414.html|title = Cobaltkieserite}}</ref><ref>{{Cite web|url=https://www.mindat.org/min-664.html|title = Bieberite}}</ref><ref name="ima-mineralogy.org">{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref>

==Health issues==

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''.<ref>{{cite journal |author= Morin Y |author2= Tětu A |author3= Mercier G|title=Quebec beer-drinkers' cardiomyopathy: Clinical and hemodynamic aspects |journal=Annals of the New York Academy of Sciences |volume=156 |issue= 1 |pages=566–576 |date=1969|pmid=5291148 |doi=10.1111/j.1749-6632.1969.tb16751.x|bibcode = 1969NYASA.156..566M |s2cid= 7422045 }}</ref><ref>{{cite journal|title = Cobalt|author = Barceloux, Donald G.|author2 = Barceloux, Donald|name-list-style = amp |doi = 10.1081/CLT-100102420|pmid = 10382556|journal = Clinical Toxicology|volume = 37|issue = 2|date = 1999| pages = 201–216}}</ref><ref>[https://pubchem.ncbi.nlm.nih.gov/compound/Cobalt_sulfate#section=Human-Toxicity-Excerpts 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).]</ref>

Furthermore, cobalt(II) sulfate is suspected of causing [[cancer]] (i.e., possibly [[carcinogen]]ic, [[IARC Group 2B]]) as per the [[International Agency for Research on Cancer]] (IARC) Monographs.<ref>{{cite web | url = http://publications.iarc.fr/_publications/media/download/2705/29aacee6b89ff816188dcd990b61a16ad6486eec.pdf | work = IARC Monographs on the Evaluation of Carcinogenic Risks to Humans | volume = 86 | title = Cobalt in Hard Metals and Cobalt Sulfate, Gallium Arsenide, Indium Phosphide and Vanadium Pentoxide }}</ref>

==Related compounds==

* the [[Tutton salt]] K₂Co(SO₄)₂{{hydrate|6|nolink=yes}}

==References==

{{reflist}}

{{Cobalt compounds}}

{{Sulfates}}

[[Category:Cobalt(II) compounds]]

[[Category:Sulfates]]

[[Category:IARC Group 2B carcinogens]]

[[Category:Hydrates]]