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(HCO2)2(H2O)2 → Ni + 2 CO2 + 2 H2O + H2

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

  1. ^ "Nickel formate".
  2. ^ a b c d e f g h Record of Nickeldiformat in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 2016-07-23.
  3. ^ a b c d e NLM Hazardous Substances Data Bank entry for [ ]
  4. ^ a b 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.
  5. ^ a b Kotz, John; Treichel, Paul; Townsend, John (2009). Chemistry and Chemical Reactivity, Enhanced Edition. Cengage Learning. p. 335. ISBN 978-0-495-39029-9.
  6. ^ Falbe, Jürgen; Regitz, Manfred (2014). RÖMPP Lexikon Chemie, 10. Auflage, 1996-1999 Band 4: M - Pk. Georg Thieme Verlag. p. 2238. ISBN 978-3-13-200031-5.
  7. ^ Werner Reutemann and Heinz Kieczka "Formic Acid" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a12_013
Allikas: https://en.wikipedia.org/wiki/Nickel_formate
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