Nickel formate
Topic: Chemistry
From HandWiki - Reading time: 2 min
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| Names | |
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| IUPAC name
nickel(2+) diformate
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| Systematic IUPAC name
nickel formate | |
| Other names
nickel diformate
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| EC Number |
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PubChem CID
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| UNII | |
| UN number | 3077 |
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| Properties | |
| C2H2NiO4 | |
| Molar mass | 148.73[2] |
| Appearance | Green Solid[2][3] |
| Odor | odourless |
| Density | 2.154 g/cm3[2] |
| Melting point | 130–140°C[2] |
| Boiling point | 180–200°C (decomposition)[2] |
| Slightly soluble in cold water[2] | |
| Solubility | insoluble in organic solvents[4] soluble in acids[3] |
| Structure | |
| monoclinic | |
| Hazards | |
| GHS pictograms |   
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| GHS Signal word | Danger |
| H317, H334, H341, H350i, H360D, H372, H410 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Nickel formate is the nickel salt of formic acid with the chemical formula Ni(HCOO)2.
Synthesis and structure
Nickel formate can be obtained by reacting nickel(II) acetate or nickel(II) hydroxide [3] with formic acid.[5]
- Ni(OH)2 + 2HCOOH → Ni(HCOO)2 + 2 H2O
Nickel formate can also be synthesized by the reaction of sodium formate with nickel (II) sulphate.[3]
Characteristics
As a dihydrate, nickel formate is a green, odorless, non-flammable solid that is sparingly soluble in water.[2] The compound has a monoclinic crystal structure.[3] The anhydride forms on careful heating at 130–140 °C.[6] When heated in a vacuum to 300 °C, pure nickel is formed:[5]
- Ni(HCO
2)
2(H
2O)
2 → Ni + 2 CO
2 + 2 H
2O + H
2
Such fine powders are useful as hydrogenation catalysts.[7]
Use
Nickel formate is used in the production of nickel and other nickel compounds such as nickel catalysts.[4]
References
- ↑ "Nickel formate". https://pubchem.ncbi.nlm.nih.gov/compound/Nickel-formate#section=Molecular-Formula.
- ↑ 2.0 2.1 2.2 2.3 2.4 2.5 2.6 2.7 Record of Nickeldiformat in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 2016-07-23.
- ↑ 3.0 3.1 3.2 3.3 3.4 Template:HSDB
- ↑ 4.0 4.1 Milne, G. W. A. (2005). Gardner's Commercially Important Chemicals Synonyms, Trade Names, and Properties. John Wiley & Sons. p. 738. ISBN 0-471-73661-9. https://books.google.com/books?id=oWdc2qcb3QsC.
- ↑ 5.0 5.1 Kotz, John; Treichel, Paul; Townsend, John (2009). Chemistry and Chemical Reactivity, Enhanced Edition. Cengage Learning. pp. 335. ISBN 978-0-495-39029-9. https://books.google.com/books?id=IBESYmQcb0sC.
- ↑ Falbe, Jürgen; Regitz, Manfred (2014). RÖMPP Lexikon Chemie, 10. Auflage, 1996-1999 Band 4: M - Pk. Georg Thieme Verlag. pp. 2238. ISBN 978-3-13-200031-5. https://books.google.com/books?id=TD3OAwAAQBAJ.
- ↑ Werner Reutemann and Heinz Kieczka "Formic Acid" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a12_013
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