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| verifiedrevid = 444024162 |
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| Name = Nickel(II) sulfate |
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| verifiedrevid = 444025273 |
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| ImageFileL1 = Nickel sulfate anh.jpg |
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| Name = Nickel(II) sulfate |
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| ImageSizeL1 = 140px |
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| ImageFileL1 = Nickel sulfate anh.jpg |
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| ImageCaptionL1 = Anhydrous |
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| ImageCaptionL1 = Anhydrous |
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| ImageFileR1 = Nickel sulfate hydrate.jpg |
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| ImageFileR1 = Nickel sulfate hydrate.jpg |
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| ImageSizeR1 = 140px |
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| ImageCaptionR1 = Hexahydrate |
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| ImageCaptionR1 = Hexahydrate |
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| ImageFile2 = N9(H2O)6SO4.png |
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| ImageFile2 = N9(H2O)6SO4.png |
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| ImageName1 = Nickel(II) sulfate hexahydrate |
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| ImageName1 = Nickel(II) sulfate hexahydrate |
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| IUPACName = Nickel(II) sulfate |
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| IUPACName = Nickel(II) sulfate |
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| OtherNames = Nickelous sulfate |
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| OtherNames = Nickelous sulfate<br>Nickel (II) sulphate |
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| Section1 = {{Chembox Identifiers |
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<!-- | Name = Safety data --> |
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| Section1 = {{Chembox Identifiers |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 22989 |
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| ChemSpiderID = 22989 |
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| ChEBI = 53001 |
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| ChEBI = 53001 |
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| SMILES = .S()(=O)=O |
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| SMILES = .S()(=O)=O |
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| SMILES_Comment = anhydrous |
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| SMILES1 = ()()()().S(=O)(=O) |
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| SMILES1_Comment = hexahydrate |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/Ni.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 |
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| StdInChI = 1S/Ni.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 |
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| CASNo = 7786-81-4 |
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| CASNo = 7786-81-4 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo_Comment = (anhydrous) |
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| CASOther = (anhydrous)<br/>10101-97-0 (hexahydrate)<br/>10101-98-1 (heptahydrate) |
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| CASNo2_Ref = {{cascite|correct|CAS}} |
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| CASNo2 = 10101-97-0 |
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| CASNo2_Comment = (hexahydrate) |
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| CASNo3_Ref = {{cascite|correct|CAS}} |
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| CASNo3 = 10101-98-1 |
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| CASNo3_Comment = (heptahydrate) |
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| UNII1_Ref = {{fdacite|correct|FDA}} |
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| UNII1 = JC9WZ4FK68 |
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| UNII1_Comment = (hexahydrate) |
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| UNII2_Ref = {{fdacite|correct|FDA}} |
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| UNII2 = 596IDD57NR |
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| UNII2_Comment = (heptahydrate) |
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| EINECS = 232-104-9 |
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| EINECS = 232-104-9 |
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| RTECS = QR9600000 |
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| RTECS = QR9600000}} |
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| Section2 = {{Chembox Properties |
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}} |
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| Section2 = {{Chembox Properties |
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| Formula = NiSO<sub>4</sub> |
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| Formula = NiSO<sub>4</sub> |
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| MolarMass = 154.75 g/mol (anhydrous)<br/>262.85 g/mol (hexahydrate) <br> 280.86 g/mol (heptahydrate) |
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| MolarMass = 154.75 g/mol (anhydrous)<br/>262.85 g/mol (hexahydrate) <br> 280.86 g/mol (heptahydrate) |
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| Appearance = yellow solid (anhydrous) <br> green crystals (hexahydrate) |
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| Appearance = yellow-green solid (anhydrous) <br> turquoise crystals (hexahydrate) <br> turquoise crystals (heptahydrate) |
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| Odor = odorless |
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| Density = 3.68 g/cm<sup>3</sup> (anhydrous) <br> 2.07 g/cm<sup>3</sup> (hexahydrate) <br> 1.948 g/cm<sup>3</sup> (heptahydrate) |
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| Solubility = 650 g/L (20°C) <br> 775 g/L (30°C) (heptahydrate) |
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| Density = 4.01 g/cm<sup>3</sup> (anhydrous) <br> 2.07 g/cm<sup>3</sup> (hexahydrate) <br> 1.948 g/cm<sup>3</sup> (heptahydrate) |
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| SolubleOther = ''anhydrous'' <br> insoluble in ], ], ] <hr> ''hexahydrate'' <br> very soluble in ], ] <hr> ''heptahydrate'' <br> soluble in ] |
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| Solubility = 65 g/100 mL (20 °C) <br> 77.5 g/100 mL (30 °C) (heptahydrate) |
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| SolubleOther = ''anhydrous'' <br> insoluble in ], ], ] <hr> ''hexahydrate'' <br> insoluble in ], ] <hr> ''heptahydrate'' <br> soluble in ] |
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| MeltingPt = > 100 °C (anhydrous) <br> 53 °C (hexahydrate) |
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| MeltingPt = 1210 °C (anhydrous, at high pressure) <br> 53 °C (hexahydrate) |
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| BoilingPt = 840 °C (anhydrous, decomp) |
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| BoilingPt = > 640 °C (anhydrous, decomposes) <br> 100 °C (hexahydrate, decomposes) |
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| RefractIndex = 1.511 (hexahydrate) <br> 1.467 (heptahydrate) |
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| RefractIndex = 1.511 (hexahydrate) <br> 1.467 (heptahydrate) |
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| pKa = 4.5 (hexahydrate) |
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}} |
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| MagSus = +4005.0·10<sup>−6</sup> cm<sup>3</sup>/mol}} |
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| Section3 = {{Chembox Structure |
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| Section3 = {{Chembox Structure |
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| Coordination = |
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| Coordination = |
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| CrystalStruct = ] (anhydrous) <br> ] (hexahydrate) <br> ] (hexahydrate) |
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| CrystalStruct = ] (anhydrous) <br> ] (hexahydrate) <br> ] (heptahydrate)}} |
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| Section7 = {{Chembox Hazards |
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}} |
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| ExternalSDS = |
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| Section7 = {{Chembox Hazards |
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| GHSPictograms = {{GHS08}} {{GHS07}} {{GHS09}} |
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| ExternalMSDS = |
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| GHSSignalWord = Danger |
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| EUIndex = 028-009-00-5 |
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| HPhrases = {{H-phrases|302+332|315|317|334|341|350|360D|372|410}} |
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| EUClass = ]<br/>]<br/>Repr. Cat. 2<br/>Toxic ('''T''')<br/>Harmful ('''Xn''')<br/>Irritant ('''Xi''')<br/>Dangerous for the environment ('''N''') |
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| PPhrases = {{P-phrases|201|261|273|280|308+313|501}} |
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| RPhrases = {{R49}}, {{R61}}, {{R20/22}}, {{R38}}, {{R42/43}}, {{R48/23}}, {{R68}}, {{R50/53}} |
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| NFPA-H = 3 |
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| SPhrases = {{S53}}, {{S45}}, {{S60}}, {{S61}} |
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| NFPA-H = |
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| NFPA-F = 0 |
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| NFPA-F = |
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| NFPA-R = 0 |
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| NFPA-R = |
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| FlashPt = Non-flammable |
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| FlashPt = Non-flammable |
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| LD50 = 264 mg/kg |
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| LD50 = 264 mg/kg}} |
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}} |
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| Section8 = {{Chembox Related |
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| OtherAnions = |
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| OtherAnions = |
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| OtherCations = ]<br/>] |
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| OtherCations = ]<br/>]<br/>]}} |
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'''Nickel(II) sulfate''', or just '''nickel sulfate''', usually refers to the ] with the ] NiSO<sub>4</sub>(H<sub>2</sub>O)<sub>6</sub>. This highly soluble blue-coloured ] is a common source of the Ni<sup>2+</sup> ion for electroplating. Nickel sulfate is ]. |
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'''Nickel(II) sulfate''', or just '''nickel sulfate''', usually refers to the ] with the ] NiSO<sub>4</sub>(H<sub>2</sub>O)<sub>6</sub>. This highly ] turquoise coloured ] is a common source of the Ni<sup>2+</sup> ] for ]. Approximately 40,000 ]s were produced in 2005.<ref name="Ullmann">K. Lascelles, L. G. Morgan, D. Nicholls, D. Beyersmann “Nickel Compounds” in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. Vol. A17 p. 235 {{doi|10.1002/14356007.a17_235.pub2}}.</ref> |
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==Structures== |
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At least seven sulfate salts of nickel(II) are known. These salts differ, sometimes subtly, in terms of their ] or structural details. The common tetragonal hexahydrate crystallizes from aqueous solution between 30.7 and 53.8 °C. Below these temperatures, a heptahydrate crystallises and above these temperatures an orthorhombic hexahydrate forms. The yellow ] form, NiSO<sub>4</sub>, is a high melting solid. This material produced by heating the hydrates above 330 °C. It decomposes at still higher temperatures to nickel oxide.<ref name=Ullmann>K. Lascelles, L. G. Morgan, D. Nicholls, D. Beyersmann “Nickel Compounds” in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. {{DOI|10.1002/14356007.a17_235.pub2}}.</ref> |
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At least seven sulfate salts of nickel(II) are known. These salts differ in terms of their ] or crystal habit. |
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The common tetragonal hexahydrate crystallizes from aqueous solution between 30.7 and 53.8 °C. Below these temperatures, a heptahydrate crystallises, and above these temperatures an orthorhombic hexahydrate forms. The yellow ] form, NiSO<sub>4</sub>, crystallizes in orthorhombic crystal system<ref>{{Cite journal |last=Dimaras |first=P. I. |date=1957-04-10 |title=Morphology and structure of anhydrous nickel sulphate |url=https://scripts.iucr.org/cgi-bin/paper?S0365110X57000900 |journal=Acta Crystallographica |volume=10 |issue=4 |pages=313–315 |doi=10.1107/S0365110X57000900|s2cid=98635639 }}</ref> and in standard pressure decomposes to ] in temperatures above 640 °C, before reaching the ].<ref>{{Cite journal |last=Tagawa |first=Hiroaki |date=October 1984 |title=Thermal decomposition temperatures of metal sulfates |url=https://linkinghub.elsevier.com/retrieve/pii/0040603184871816 |journal=Thermochimica Acta |language=en |volume=80 |issue=1 |pages=23–33 |doi=10.1016/0040-6031(84)87181-6}}</ref> It melts only at high system pressure, using a constant volume method the melting point was found to be 1210 °C.<ref>{{Cite journal |last1=Kobertz |first1=Dietmar |last2=Müller |first2=Michael |date=June 2014 |title=Experimental studies on NiSO4 by thermal analysis and calorimetry |url=https://linkinghub.elsevier.com/retrieve/pii/S0364591613001041 |journal=Calphad |language=en |volume=45 |pages=55–61 |doi=10.1016/j.calphad.2013.10.008}}</ref> The anhydrous sulfate is produced by heating the hydrates above 330 °C. |
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] measurements show that NiSO<sub>4</sub>·6H<sub>2</sub>O consists of the octahedral <sup>2+</sup> ions. These ions in turn are ]ed to sulfate ions.<ref>Wells, A. F. (1984). Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.</ref> Dissolution of the salt in water gives solutions containing the ] <sup>2+</sup>. |
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] measurements show that NiSO<sub>4</sub>·6H<sub>2</sub>O consists of the octahedral {{chem2|(2+)}} ions. These ions in turn are ]ed to sulfate ions.<ref>Wells, A. F. (1984). Structural Inorganic Chemistry, Oxford: Clarendon Press. {{ISBN|0-19-855370-6}}.</ref> Dissolution of the salt in water gives solutions containing the ] {{chem2|(2+)}}. |
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All nickel sulfates are ]. |
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==Production, applications, and coordination chemistry== |
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==Production, applications, and coordination chemistry== |
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The salt is usually obtained as a by-product of ]. It is also produced by dissolution of nickel metal or nickel oxides in sulfuric acid. Approximately 40,000 tonnes were produced in 2005. It is mainly used for electroplating of nickel.<ref name=Ullmann/> |
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The salt is usually obtained as a by-product of ]. It can also be produced by dissolution of nickel metal or nickel oxides in sulfuric acid. |
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Aqueous solutions of nickel sulfate reacts with sodium carbonate to precipitate ], a precursor to nickel-based catalysts and pigments. Addition of ] to concentrated aqueous solutions of nickel sulfate precipitates Ni(NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub>·6H<sub>2</sub>O. This blue-coloured solid is analogous to ], Fe(NH<sub>4</sub>)<sub>2</sub>SO<sub>4</sub>·6H<sub>2</sub>O.<ref name=Ullmann/> |
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Aqueous solutions of nickel sulfate react with sodium carbonate to precipitate ], a precursor to nickel-based catalysts and pigments.<ref>H. B. W. Patterson, "Catalysts" in Hydrogenation of Fats and Oils G. R. List and J. W. King, Eds., 1994, AOCS Press, Urbana.</ref> Addition of ] to concentrated aqueous solutions of nickel sulfate precipitates {{chem2|Ni(NH4)2(SO4)2*6H2O}}. This blue-coloured solid is analogous to ], {{chem2|Fe(NH4)2(SO4)2*6H2O}}.<ref name=Ullmann/> |
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Nickel sulfate is used in the laboratory. Columns used in ]ging, useful in ] and ], are regenerated with nickel sulfate. Aqueous solutions of NiSO<sub>4</sub>·6H<sub>2</sub>O and related hydrates react with ammonia to give SO<sub>4</sub> and with ] to give SO<sub>4</sub>. The latter is occasionally used as a calibrant for ] measurements because it has no tendency to hydrate. |
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Nickel sulfate has some uses in the laboratory. Columns used in ]ging, useful in ] and ], are regenerated with nickel sulfate. Aqueous solutions of NiSO<sub>4</sub>·6H<sub>2</sub>O and related hydrates react with ammonia to give {{chem2|SO4}} and with ] to give the ] {{chem2|SO4}}. The latter is occasionally used as a calibrant for ] measurements because it has no tendency to hydrate. |
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==Natural occurrence== |
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==Natural occurrence== |
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Nickel sulfate occurs as the rare mineral ], which is a hexahydrate. The second hexahydrate is known as ] (Ni,Mg,Fe)SO<sub>4</sub>·6H<sub>2</sub>O. The heptahydrate, which is relatively unstable in air, occurs as ]. The monohydrate occurs as very rare mineral ] (Ni,Fe)SO<sub>4</sub>·H<sub>2</sub>O. |
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Nickel sulfate occurs as the rare mineral retgersite,<ref>{{Cite web |title=Retgersite |url=https://www.mindat.org/min-3489.html |website=mindat.org}}</ref> which is a ]. The second hexahydrate is known as nickelhexahydrite {{chem2|(Ni,Mg,Fe)SO4*6H2O}}, which is the monoclinic dimorph of retgersite. The heptahydrate, which is relatively unstable in air, occurs as morenosite. The monohydrate occurs as the very rare mineral dwornikite {{chem2|(Ni,Fe)SO4*H2O}}. |
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==Safety== |
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==Safety== |
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Nickel salts are ]ic and irritate the skin. |
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In 2005–2006, nickel sulfate was the top ] in ]s (19.0%).<ref name="Zug KA 2006">Zug KA, Warshaw EM, Fowler JF Jr, Maibach HI, Belsito DL, Pratt MD, Sasseville D, Storrs FJ, Taylor JS, Mathias CG, Deleo VA, Rietschel RL, Marks J. Patch-test results of the North American Contact Dermatitis Group 2005–2006. Dermatitis. 2009 May–Jun;20(3):149-60.</ref> Nickel sulfate is classified as a human carcinogen<ref>IARC (2012). “Nickel and nickel compounds” ''IARC Monogr Eval Carcinog Risks Hum,'' Volume 100C: 169-218.'' ''</ref><ref>NTP (National Toxicology Program). 2016. “Report on Carcinogens”, 14th Edition.; Research Triangle Park, NC: U.S. Department of Health and Human Services, Public Health Service. https://ntp.niehs.nih.gov/pubhealth/roc/index-1.html Accessed July 13, 2017.</ref> based on increased respiratory cancer risks observed in epidemiological studies of sulfidic ore refinery workers.<ref>International Committee on Nickel Carcinogenesis in Man (ICNCM). (1990). Report of the International Committee on Nickel Carcinogenesis in Man. ''Scan. J. Work Environ. Health.'' '''16(1):''' 1-82.</ref> In a 2-year inhalation study in F344 rats and B6C3F1 mice, there was no evidence of carcinogenic activity, although increased lung inflammations and bronchial ] hyperplasia were observed.<ref>National Toxicology Program (NTP). (1996). Toxicology and Carcinogenesis Studies of Nickel Sulfate Hexahydrate (CAS NO. 10101-97-0) in F344/N Rats and B6CF1 Mice (Inhalation Studies). US DHHS. ''NTP TR 454.'' NIH Publication No. 96-3370.</ref> These results strongly suggest that there is a threshold for the carcinogenicity of nickel sulfate via inhalation. In a 2-year study with daily oral administration of nickel sulfate hexahydrate to F344 rats, no evidence for increased carcinogenic activity was observed.<ref>Heim, K. E.; Bates, H. K.; Rush, R. E.; Oller, A. R. (2007). “Oral Carcinogenicity Study with Nickel Sulfate Hexahydrate in Fischer 344 Rats.” ''Toxicol. Appl. Pharmacol.'' '''224(2):''' 126-137.</ref> The human and animal data consistently indicate a lack of carcinogenicity via the oral route of exposure and limit the carcinogenicity of nickel compounds to respiratory tumours after inhalation.<ref>Cogliano, V. J.; Baan, R.; Straif, K.; Grosse, Y.; Lauby-Secretan, B.; Ghissassi, F. E.; Bouvard, V.; Benbrahim-Tallaa, L.; Guha, N.; Freeman, C.; Galichet, L.; Wild, C. P. (2011). “Preventable Exposures Associated With Human Cancers”. ''J Natl Cancer Inst'' '''103:''' 1827-1839.</ref> Whether these effects are relevant to humans is unclear as epidemiological studies of highly exposed female workers have not shown adverse developmental toxicity effects.<ref>Vaktskjold, A.; Talykova, L. V.; Chashchin, V. P.; Odland, J. O.; Nieboer, E. (2008). “Spontaneous abortions among nickel-exposed female refinery workers.” ''Int J Environ Health Res.'' '''18(2):''' 99-115.</ref> |
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==References== |
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==References== |
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==External links== |
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==External links== |
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{{Commons cat|Nickel(II) sulfate}} |
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{{Commons category|Nickel(II) sulfate}} |
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{{Nickel compounds}} |
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{{Sulfates}} |
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