| IUPAC name
| Other names
|Molar mass||63.06 g/mol|
|Appearance||White hygroscopic solid|
|Melting point||116 °C (241 °F; 389 K)|
|Boiling point||180 °C (356 °F; 453 K) (decomposes)|
| 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, diethyl ether, ethanol, methanol|
Insoluble in benzene
Std enthalpy of
|Safety data sheet||ScienceLab|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|410 mg/kg (mice, intravenous)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Ammonium formate is an organic chemical compound, an ammonium salt of formic acid. It is a colorless, hygroscopic solid, with the chemical formula NH4HCOO.
Heating ammonium formate will cause it to convert it into formamide:
- NH4HCO2 → HCONH2 + H2O
- HC(O)NH2 → CO + NH3
- HC(O)NH2 → HCN + H2O
Ammonium formate can be used in the reductive amination of aldehydes and ketones, process known as Leuckart reaction.
- HCOONH4 + (CH3)2CO → (CH3)2HC-NH2 + H2O + CO2
Ammonium formate is a hygroscopic white crystalline solid, soluble in water.
Ammonium formate is sold by big chemical suppliers, while smaller suppliers rarely have it in their stock.
Ammonium formate can be made by bubbling ammonia through formic acid, though this requires lots of ammonia. An ammonium salt, such as ammonium bicarbonate can be used instead. Cooling the solution will cause the salt to precipitate. Excess water can be evaporated by carefully heating the solution, at below 115 °C, to prevent it from melting/decomposing. Filter the resulting precipitate and leave it to dry, either in open air or in a desiccator. Heating is not recommended as it will cause it to decompose.
- Make formamide
- Make isopropylamine and other amines from ketones
Ammonium formate may release formic acid vapors and protection should be worn when handling the compound.
Ammonium formate should be kept in closed bottles, away from moisture. Ammonia may be added to limit hydrolysis.
Mixing it with an alkali will neutralize it.