Nickel(II) sulfate, or just nickel sulfate, usually refers to the inorganic compound with the formula NiSO4(H2O)6. This highly soluble blue green coloured salt is a common source of the Ni2+ion for electroplating.
At least seven sulfate salts of nickel(II) are known. These salts differ in terms of their hydration or crystal habit.
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 anhydrous form, NiSO4, crystallizes in orthorhombic crystal system[2] and in standard pressure decomposes to NiO in temperatures above 640 °C, before reaching the melting point.[3] It melts only at high system pressure, using a constant volume method the melting point was found to be 1210 °C.[4] The anhydrous sulfate is produced by heating the hydrates above 330 °C.
X-ray crystallography measurements show that NiSO4·6H2O consists of the octahedral [Ni(H2O)6]2+ ions. These ions in turn are hydrogen bonded to sulfate ions.[5] Dissolution of the salt in water gives solutions containing the aquo complex[Ni(H2O)6]2+.
Production, applications, and coordination chemistryedit
The salt is usually obtained as a by-product of copper refining. It is also produced by dissolution of nickel metal or nickel oxides in sulfuric acid.
Aqueous solutions of nickel sulfate reacts with sodium carbonate to precipitate nickel carbonate, a precursor to nickel-based catalysts and pigments.[6] Addition of ammonium sulfate to concentrated aqueous solutions of nickel sulfate precipitates Ni(NH4)2(SO4)2·6H2O. This blue-coloured solid is analogous to Mohr's salt, Fe(NH4)2(SO4)2·6H2O.[1]
Nickel sulfate is used in the laboratory. Columns used in polyhistidine-tagging, useful in biochemistry and molecular biology, are regenerated with nickel sulfate. Aqueous solutions of NiSO4·6H2O and related hydrates react with ammonia to give [Ni(NH3)6]SO4 and with ethylenediamine to give [Ni(H2NCH2CH2NH2)3]SO4. The latter is occasionally used as a calibrant for magnetic susceptibility measurements because it has no tendency to hydrate.
Natural occurrenceedit
Nickel sulfate occurs as the rare mineral retgersite, which is a hexahydrate. The second hexahydrate is known as nickelhexahydrite (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 (Ni,Fe)SO4·H2O.
In 2005–2006, nickel sulfate was the top allergen in patch tests (19.0%).[7] Nickel sulfate is classified as a human carcinogen[8][9][10][11] based on increased respiratory cancer risks observed in epidemiological studies of sulfidic ore refinery workers.[12] 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 lymph node hyperplasia were observed.[13] 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.[14] 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.[15] Whether these effects are relevant to humans is unclear as epidemiological studies of highly exposed female workers have not shown adverse developmental toxicity effects.[16]
Referencesedit
^ abK. 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.
^Dimaras, P. I. (1957-04-10). "Morphology and structure of anhydrous nickel sulphate". Acta Crystallographica. 10 (4): 313–315. doi:10.1107/S0365110X57000900. S2CID 98635639.
^Tagawa, Hiroaki (October 1984). "Thermal decomposition temperatures of metal sulfates". Thermochimica Acta. 80 (1): 23–33. doi:10.1016/0040-6031(84)87181-6.
^Kobertz, Dietmar; Müller, Michael (June 2014). "Experimental studies on NiSO4 by thermal analysis and calorimetry". Calphad. 45: 55–61. doi:10.1016/j.calphad.2013.10.008.
^Wells, A. F. (1984). Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN0-19-855370-6.
^H. B. W. Patterson, "Catalysts" in Hydrogenation of Fats and Oils G. R. List and J. W. King, Eds., 1994, AOCS Press, Urbana.
^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.
^Regulation (EC) No 1272/2008 of the European Parliament and of the Council of 16 December 2008 on Classification, Labelling and Packaging of Substances and Mixtures, Amending and Repealing Directives 67/548/EEC and 1999/45/EC and amending Regulation (EC) No 1907/2006
^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.
^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.
^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.
^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.
^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 Inst103: 1827-1839.
^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.
External linksedit
Wikimedia Commons has media related to Nickel(II) sulfate.
International Chemical Safety Card 0063
February 15, 2024
nickel, sulfate, just, nickel, sulfate, usually, refers, inorganic, compound, with, formula, niso4, this, highly, soluble, blue, green, coloured, salt, common, source, electroplating, anhydrous, hexahydratenamesiupac, name, other, names, nickelous, sulfatenick. Nickel II sulfate or just nickel sulfate usually refers to the inorganic compound with the formula NiSO4 H2O 6 This highly soluble blue green coloured salt is a common source of the Ni2 ion for electroplating Nickel II sulfate Anhydrous HexahydrateNamesIUPAC name Nickel II sulfateOther names Nickelous sulfateNickel II sulphateIdentifiersCAS Number 7786 81 4 anhydrous Y10101 97 0 hexahydrate Y10101 98 1 heptahydrate Y3D model JSmol Interactive imageChEBI CHEBI 53001 YChemSpider 22989 YECHA InfoCard 100 029 186EC Number 232 104 9PubChem CID 24586RTECS number QR9600000UNII 4FLT4T3WUN YJC9WZ4FK68 hexahydrate Y596IDD57NR heptahydrate YCompTox Dashboard EPA DTXSID6023787InChI InChI 1S Ni H2O4S c 1 5 2 3 4 h H2 1 2 3 4 q 2 p 2 YKey LGQLOGILCSXPEA UHFFFAOYSA L YInChI 1 Ni H2O4S c 1 5 2 3 4 h H2 1 2 3 4 q 2 p 2Key LGQLOGILCSXPEA NUQVWONBAGSMILES Ni 2 O S O O OPropertiesChemical formula NiSO4Molar mass 154 75 g mol anhydrous 262 85 g mol hexahydrate 280 86 g mol heptahydrate Appearance yellow solid anhydrous blue crystals hexahydrate green blue crystals heptahydrate Odor odorlessDensity 4 01 g cm3 anhydrous 2 07 g cm3 hexahydrate 1 948 g cm3 heptahydrate Melting point 1210 C anhydrous at high pressure 53 C hexahydrate Boiling point gt 640 C anhydrous decomposes 100 C hexahydrate decomposes Solubility in water 65 g 100 mL 20 C 77 5 g 100 mL 30 C heptahydrate Solubility anhydrous insoluble in ethanol ether acetone hexahydrate insoluble in ethanol ammonia heptahydrate soluble in alcoholAcidity pKa 4 5 hexahydrate Magnetic susceptibility x 4005 0 10 6 cm3 molRefractive index nD 1 511 hexahydrate 1 467 heptahydrate StructureCrystal structure orthorombic anhydrous tetragonal hexahydrate rhombohedral heptahydrate HazardsGHS labelling PictogramsSignal word DangerHazard statements H302 H332 H315 H317 H334 H341 H350 H360D H372 H410Precautionary statements P201 P261 P273 P280 P308 P313 P501NFPA 704 fire diamond 300Flash point Non flammableLethal dose or concentration LD LC LD50 median dose 264 mg kgSafety data sheet SDS External MSDSRelated compoundsOther cations Cobalt II sulfateCopper II sulfateIron II sulfateExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa N verify what is Y N Infobox references Approximately 40 000 tonnes were produced in 2005 It is mainly used for electroplating of nickel 1 Contents 1 Structures 2 Production applications and coordination chemistry 3 Natural occurrence 4 Safety 5 References 6 External linksStructures edit nbsp Nickel sulfate hexahydrate under a microscope At least seven sulfate salts of nickel II are known These salts differ in terms of their hydration or crystal habit 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 anhydrous form NiSO4 crystallizes in orthorhombic crystal system 2 and in standard pressure decomposes to NiO in temperatures above 640 C before reaching the melting point 3 It melts only at high system pressure using a constant volume method the melting point was found to be 1210 C 4 The anhydrous sulfate is produced by heating the hydrates above 330 C X ray crystallography measurements show that NiSO4 6H2O consists of the octahedral Ni H2O 6 2 ions These ions in turn are hydrogen bonded to sulfate ions 5 Dissolution of the salt in water gives solutions containing the aquo complex Ni H2O 6 2 All nickel sulfates are paramagnetic Production applications and coordination chemistry editThe salt is usually obtained as a by product of copper refining It is also produced by dissolution of nickel metal or nickel oxides in sulfuric acid Aqueous solutions of nickel sulfate reacts with sodium carbonate to precipitate nickel carbonate a precursor to nickel based catalysts and pigments 6 Addition of ammonium sulfate to concentrated aqueous solutions of nickel sulfate precipitates Ni NH4 2 SO4 2 6H2O This blue coloured solid is analogous to Mohr s salt Fe NH4 2 SO4 2 6H2O 1 Nickel sulfate is used in the laboratory Columns used in polyhistidine tagging useful in biochemistry and molecular biology are regenerated with nickel sulfate Aqueous solutions of NiSO4 6H2O and related hydrates react with ammonia to give Ni NH3 6 SO4 and with ethylenediamine to give Ni H2NCH2CH2NH2 3 SO4 The latter is occasionally used as a calibrant for magnetic susceptibility measurements because it has no tendency to hydrate Natural occurrence editNickel sulfate occurs as the rare mineral retgersite which is a hexahydrate The second hexahydrate is known as nickelhexahydrite 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 Ni Fe SO4 H2O Safety edit nbsp Patch testIn 2005 2006 nickel sulfate was the top allergen in patch tests 19 0 7 Nickel sulfate is classified as a human carcinogen 8 9 10 11 based on increased respiratory cancer risks observed in epidemiological studies of sulfidic ore refinery workers 12 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 lymph node hyperplasia were observed 13 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 14 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 15 Whether these effects are relevant to humans is unclear as epidemiological studies of highly exposed female workers have not shown adverse developmental toxicity effects 16 References edit a b 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 Dimaras P I 1957 04 10 Morphology and structure of anhydrous nickel sulphate Acta Crystallographica 10 4 313 315 doi 10 1107 S0365110X57000900 S2CID 98635639 Tagawa Hiroaki October 1984 Thermal decomposition temperatures of metal sulfates Thermochimica Acta 80 1 23 33 doi 10 1016 0040 6031 84 87181 6 Kobertz Dietmar Muller Michael June 2014 Experimental studies on NiSO4 by thermal analysis and calorimetry Calphad 45 55 61 doi 10 1016 j calphad 2013 10 008 Wells A F 1984 Structural Inorganic Chemistry Oxford Clarendon Press ISBN 0 19 855370 6 H B W Patterson Catalysts in Hydrogenation of Fats and Oils G R List and J W King Eds 1994 AOCS Press Urbana 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 IARC 2012 Nickel and nickel compounds IARC Monogr Eval Carcinog Risks Hum Volume 100C 169 218 Regulation EC No 1272 2008 of the European Parliament and of the Council of 16 December 2008 on Classification Labelling and Packaging of Substances and Mixtures Amending and Repealing Directives 67 548 EEC and 1999 45 EC and amending Regulation EC No 1907 2006 Globally Harmonised System of Classification and Labelling of Chemicals GHS Fifth revised edition United Nations New York and Geneva 2013 PDF at https www unece org fileadmin DAM trans danger publi ghs ghs rev05 English ST SG AC10 30 REv5e pdf Accessed July 13 2017 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 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 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 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 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 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 External links edit nbsp Wikimedia Commons has media related to Nickel II sulfate International Chemical Safety Card 0063 Retrieved from https en wikipedia org w index php title Nickel II sulfate amp oldid 1180629570, wikipedia, wiki, book, books, library,
