Ammonium formate

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Ammonium formate
Skeletal formula of ammonium formate
Ball-and-stick model of ammonium formate
IUPAC name
Ammonium formate
3D model (JSmol)
ECHA InfoCard 100.007.959
RTECS number BQ6650000
Molar mass 63.056 g·mol−1
Appearance White monoclinic crystals, deliquescent
Odor Slightly ammoniac
Density 1.26 g/cm3[1]
Melting point 116 °C (241 °F; 389 K)
Boiling point 180 °C (356 °F; 453 K)
(grams per 100g of water)102g(0 °C)
142.7 g (20 °C)
202.4 g (40 °C)
516 g (80 °C)[2]
Solubility in other solvents Soluble in liquid ammonia, alcohol, diethyl ether[2]
−556.18 kJ/mol
Safety data sheet JT Baker MSDS
GHS pictograms GHS07: Harmful[1]
GHS signal word Warning
H315, H319, H335[1]
P261, P305+351+338[1]
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oilHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroformReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calciumSpecial hazards (white): no codeNFPA 704 four-colored diamond
Lethal dose or concentration (LD, LC):
410 mg/kg (mice, intravenous)[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Ammonium formate, NH4HCO2, is the ammonium salt of formic acid. It is a colorless, hygroscopic, crystalline solid.

Reductive amination[edit]

Acetone can be transformed into isopropylamine as follows:[citation needed]

CH3C(O)CH3 + 2 HCO2 +NH4 → (CH3)2CHNHCHO + 2 H2O + NH3 + CO2


Pure ammonium formate decomposes into formamide and water when heated, and this is its primary use in industry. Formic acid can also be obtained by reacting ammonium formate with a dilute acid, and since ammonium formate is also produced from formic acid, it can serve as a way of storing formic acid.

Ammonium formate can also be used in palladium on carbon (Pd/C) reduction of functional groups. In the presence of Pd/C, ammonium formate decomposes to hydrogen, carbon dioxide, and ammonia. This hydrogen gas is adsorbed onto the surface of the palladium metal, where it can react with various functional groups. For example, alkenes can be reduced to alkanes, or formaldehyde to methanol. Activated single bonds to heteroatoms can also be replaced by hydrogens (hydrogenolysis).

Ammonium formate can be used for reductive amination of aldehydes and ketones (Leuckart reaction), by the following reaction:[3]

The Leuckart reaction scheme-.svg

Ammonium formate can be used as a buffer in high performance liquid chromatography (HPLC), and is suitable for use with liquid chromatography-mass spectrometry (LC/MS). The pKa values of formic acid and the ammonium ion are 3.8 and 9.2, respectively.


When heated, ammonium formate eliminates water, forming formamide. Upon further heating, it forms hydrogen cyanide (HCN) and water. A side reaction of this is the decomposition of formamide to carbon monoxide (CO) and ammonia.


  1. ^ a b c d Sigma-Aldrich Co., Ammonium formate. Retrieved on 2014-06-10.
  2. ^ a b c d
  3. ^ Alexander, Elliot; Ruth Bowman Wildman (1948). "Studies on the Mechanism of the Leuckart Reaction". Journal of the American Chemical Society. 70: 1187–1189. doi:10.1021/ja01183a091.

External links[edit]

Media related to Ammonium formate at Wikimedia Commons