Nickel(II) sulfate

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Nickel(II) Sulfate
IUPAC name
Nickel(II) sulfate
Other names
Nickelous sulfate
Identifiers
CAS number
7786-81-4,(anhydrous)10101-97-0 (hexahydrate)10101-98-1 (heptahydrate)
EC number
232-104-9
RTECS number
QR9600000
Properties
Molecular formula
NiSO4
Molar mass
154.75 g/mol (anhydrous)262.85 g/mol (hexahydrate)
Appearance
Blue crystals (hexahydrate)Yellow powder (anhydrous)
Density
3.68 g/cm3 (anhydrous)2.07 g/cm3 (hexahydrate)
Melting point
> 100 (anhydrous)53 (hexahydrate)
Boiling point
840 (anhydrous)
Solubility in water
65.0 g/100mL (20)77.5 g/100mL (30)
Solubility in ethanol
sparingly (hexahydrate)
Structure
Crystal structure
tetragonal
Hazards
MSDS
External MSDS
EU classification
Carc. Cat. 1Muta. Cat. 3Repr. Cat. 2Toxic (T)Harmful (Xn)Irritant (Xi)Dangerous for the environment (N)
EU Index
028-009-00-5
R-phrases
R49, R61, R20/22, R38, R42/43, R48/23, R68, R50/53
S-phrases
S53, S45, S60, S61
Flash point
Non-flammable
LD50
264 mg/kg
Related compounds
Other cations
Cobalt(II) sulfateCopper(II) sulfate
Except where noted otherwise, data are given formaterials in their standard state(at 25, 100kPa)Infobox references
Nickel(II) sulfate, or just nickel sulfate, usually refers to the chemical compound with the formula NiSO4. This highly soluble blue-coloured salt is a common source of the Ni2+ ion for electroplating.
Several sulfate salts of nickel(II) are known, all being paramagnetic. These salts differ with respect to their hydration or subtle structural details. The common tetragonal hexahydrate crystallizes from aqueous solution between 30.7 and 53.8 . Below these temperatures, a heptahydrate crystallises and above these temperatures an orthorhombic hexahydrate forms. The yellow anhydrous form, NiSO4, is a high melting solid. This material produced by heating the hydrates above 330 . It decomposes at still higher temperatures to nickel oxide.[1]
X-ray crystallography measurements show that NiSO46H2O consists of octahedral [Ni(H2O)6]2+ ions. These ions in turn are hydrogen bonded to sulfate ions.[2] Dissolution of the salt in water gives solutions containing the ion [Ni(H2O)6]2+.
Contents
1 Production, applications, and coordination chemistry
2 Natural occurrence
3 Safety
4 References
5 External links
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Production, applications, and coordination chemistry

An aqueous solution of nickel sulfate hexahydrate.
The salt is usually obtained by dissolution of nickel metal or nickel oxides in sulfuric acid. Approximately 10,000 tonnes were produced in 2005. It is mainly used to for electroplating of nickel.
Aqueous solutions of nickel sulfate reacts with sodium carbonate to precipitate nickel carbonate, a precursor to nickel-based catalysts and pigments. Addition of ammonium sulfate to concentrated aqueous solutions of nickel sulfate precipitates Ni(NH4)2SO46H2O. This blue-coloured solid is analogous to Mohr's salt, Fe(NH4)2SO46H2O.[1]
Aqueous solutions of NiSO46H2O 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
Nickel sulfate occurs as the rare mineral retgersite, which is a hexahydrate. The second hexahydrate is known as nickelhexahydrite (Ni,Mg,Fe)SO46H2O. The heptahydrate, which is relatively unstable in air, occurs as morenosite. The monohydrate occurs as very rare mineral dwornikite (Ni,Fe)SO42O.
Safety
Nickel salts are carcinogenic, and this salt is a skin irritant
References
^ a b K. Lascelles, L. G. Morgan, D. Nicholls, D. Beyersmann ickel Compounds in Ullmann's Encyclopedia of Industrial Chemistry 2005 Wiley-VCH, Weinheim, 2005.
^ Wells, A. F. (1984). Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
External links
International Chemical Safety Card 0063

v?d?eNickel compounds
NiBr2 NiCO3 Ni(CO)4 NiCl2 NiCrO4 NiF2 NiI2 Ni(NO3)2 NiO Ni(OH)2 NiSO4 Ni2O3
Categories: Nickel compounds | Sulfates | IARC Group 1 carcinogens(and so on)

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