| IUPAC name
| Preferred IUPAC name
| Systematic IUPAC name
| Other names
Hydrogen carboxylic acid
|Molar mass||46.03 g/mol|
|Density||1.220 g/cm3 (20 °C)|
|Melting point||8.4 °C (47.1 °F; 281.5 K)|
|Boiling point||100.8 °C (213.4 °F; 373.9 K)|
|Solubility|| Reacts with amines|
Miscible with acetone, diethyl ether, ethanol, ethyl acetate, glycerol, methanol
Partially soluble in benzene, toluene, xylene
|Vapor pressure||35 mmHg (20 °C)|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich (85% solution)|
|Flash point||69 °C (156 °F; 342 K)|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
| 700 mg/kg (mouse, oral)|
1,100 mg/kg (rat, oral)
4,000 mg/kg (dog, oral)
LC50 (Median concentration)
| 7,853 ppm (rat, 15 min)|
3,246 ppm (mouse, 15 min)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Formic acid or methanoic acid is an organic compound with chemical formula HCOOH and the simplest carboxylic acid.
Formic acid is readily dehydrated by concentrated sulfuric acid to carbon monoxide, and is often used in the lab as a convenient and store-able source of the gas. As with other carboxylic acids, formic acid is easily esterified with primary alcohols, often forming pleasant-smelling compounds such as methyl formate. Being a strong acid, esterifications with formic acid generally don't require an acid catalyst.
In organic chemistry, formic acid is used to introduce a formyl group.
Formic acid is a clear liquid with a highly irritating pungent odor, and is responsible for the painful sensation of many ant stings. Its boiling point is nearly the same as water (100.8 ˚C), though it forms an azeotrope of 22.4% formic acid with water that boils instead at 107.3 ˚C.
Since formic acid slowly decomposes when boiled, distillation must be done at low temperature and in near vacuum (25°C at 40 mm Hg).
While not typically found as a consumer product, formic acid can be bought online for relatively low prices, typically mixed with about 5-10% water. A good supplier is Duda Diesel.
Formic acid can also be purchased at beekeeping stores, as 60-85% concentration. It is used for the treatment of Varroasis.
Aqueous formic acid can be distilled from a mixture of anhydrous glycerol and oxalic acid, producing carbon dioxide as a byproduct. It can also be obtained by acidifying sodium formate with dilute sulfuric acid, producing formic acid in solution that can then be distilled over. Using concentrated sulfuric acid or heating too much will produce carbon monoxide and potentially create a very dangerous situation.
- Make formate esters
- Generate carbon monoxide for reactions
- Formic anhydride synthesis (stable only as solution in diethyl ether)
Concentrated solutions of formic acid are corrosive to human skin, as well as nose, mouth and eyes and also slowly decompose to form water and carbon monoxide, which can cause an explosion from pressure buildup in a sealed container. Adding a dehydrating agent will also generate large amounts of carbon monoxide, a deadly gas that is impossible to detect with human senses. Formic acid is not inherently very toxic if ingested, though long exposure to it by any means can cause chronic bodily effects. It is especially important that formic acid is kept away from the eyes, as it readily damages the optic nerve and can cause permanent blindness.
Formic acid should be stored in closed bottles, away from any heat source.
Formic acid should be neutralized before disposal. Any base can be used.
- Purification of Laboratory Chemicals (Fifth Edition), Wilfred L.F. Armarego and Christina Li Lin Chai, 2003