|Jmol-3D images||Image 1
|Molar mass||63.06 g mol−1|
|Appearance||White monoclinic crystals, deliquescent|
|Melting point||116 °C (241 °F; 389 K)|
|Boiling point||180 °C (356 °F; 453 K)
|Solubility in water||102 g/100 mL (0 °C)
142.7 g/100 mL (20 °C)
202.4 g/100 mL (40 °C)
516 g/100 mL (80 °C)
|Solubility||Soluble in liquid ammonia, alcohol, diethyl ether|
|Std enthalpy of
|MSDS||JT Baker MSDS|
|GHS signal word||Warning|
|GHS hazard statements||H315, H319, H335|
|GHS precautionary statements||P261, P305+351+338|
|LD50||410 mg/kg (mice, intravenous)|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
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 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.
- Sigma-Aldrich Co., Ammonium formate. Retrieved on 2014-06-10.
- 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.
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