View source for Formic acid

{{Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 443825627
| Name = Formic acid
| ImageFile2 = formic acid 85 percent.jpg
| ImageSize2 = 120px
| ImageFileL1 = Formic_acid.svg
| ImageNameL1 = Skeletal structure of formic acid
| ImageFileR1 = Formic-acid-CRC-MW-3D-balls.png
| ImageNameR1 = 3D model of formic acid
| PIN = Formic acid<ref name=iupac2013>{{cite book | title =  Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book) | publisher = [[Royal Society of Chemistry|The Royal Society of Chemistry]] | date = 2014 | location = Cambridge | page = 745 | doi = 10.1039/9781849733069 | isbn = 978-0-85404-182-4| last1 = Favre | first1 = Henri A. | last2 = Powell | first2 = Warren H. }}</ref>
| SystematicName = Methanoic acid<ref name=iupac2013 />
| OtherNames = Carbonous acid; Formylic acid; Hydrogen carboxylic acid; Hydroxy(oxo)methane; Metacarbonoic acid; Oxocarbinic acid; Oxomethanol
|Section1={{Chembox Identifiers
| DrugBank_Ref = {{drugbankcite|correct|drugbank}}
| DrugBank = DB01942
| SMILES = O=CO
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 0YIW783RG1
| KEGG_Ref = {{keggcite|correct|kegg}}
| KEGG = C00058
| InChI = 1/HCOOH/c2-1-3/h1H,(H,2,3)
| InChIKey = BDAGIHXWWSANSR-UHFFFAOYAT
| ChEMBL_Ref = {{ebicite|correct|EBI}}
| ChEMBL = 116736
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChI = 1S/HCOOH/c2-1-3/h1H,(H,2,3)
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = BDAGIHXWWSANSR-UHFFFAOYSA-N
| CASNo = 64-18-6
| CASNo_Ref = {{cascite|correct|CAS}}
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 30751
| PubChem = 284
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 278
| RTECS = LQ4900000
| EINECS = 200-579-1
 }}
|Section2={{Chembox Properties
| C=1 | H=2 | O=2
| Appearance = Colorless fuming liquid
| Odor = Pungent, penetrating
| Density = 1.220 g/mL
| Solubility = Miscible
| SolubleOther = Miscible with [[ether]], [[acetone]], [[ethyl acetate]], [[glycerol]], [[methanol]], [[ethanol]] <br/> Partially soluble in [[benzene]], [[toluene]], [[xylene]]s
| MeltingPtC = 8.4
| BoilingPtC = 100.8
| pKa = 3.77<ref>Brown, H. C. et al., in Braude, E. A. and Nachod, F. C., ''Determination of Organic Structures by Physical Methods'', Academic Press, New York, 1955.</ref>
| ConjugateBase = [[Formate]]
| Viscosity = 1.57 c[[Poise (unit)|P]] at 268&nbsp;°C
| LogP = −0.54
| RefractIndex = 1.3714 (20&nbsp;°C)
| MagSus = -19.90·10<sup>−6</sup> cm<sup>3</sup>/mol
| VaporPressure = 35 mmHg (20&nbsp;°C)<ref name=PGCH/>
 }}
|Section3={{Chembox Structure
| MolShape = [[Wiktionary:planar|Planar]]
| Dipole = 1.41 [[Debye|D]] (gas)}}
|Section5={{Chembox Thermochemistry
| DeltaHf = &minus;425.0 kJ/mol
| DeltaHc = &minus;254.6 kJ/mol
| Entropy = 131.8 J/mol&nbsp;K
 }}
|Section6={{Chembox Pharmacology
| ATCvet = yes
| ATCCode_prefix = P53
| ATCCode_suffix = AG01
}}
|Section7={{Chembox Hazards
| ExternalSDS = [http://www.jtbaker.com/msds/englishhtml/f5956.htm JT Baker]
| MainHazards = Corrosive; irritant;<br />sensitizer
| NFPA-H = 3
| NFPA-F = 2
| NFPA-R = 1
| FlashPtC = 69
| AutoignitionPtC = 601
| ExploLimits = 14{{ndash}}34%{{citation needed|date=March 2015}}<br/> 18%{{ndash}}57% (90% solution)<ref name=PGCH/>
| RPhrases = {{R10}} {{R35}}
| SPhrases = {{S1/2}} {{S23}} {{S26}} {{S45}}
| LD50 = 700 mg/kg (mouse, oral), 1100 mg/kg (rat, oral), 4000 mg/kg (dog, oral)<ref name=IDLH>{{cite web |url = https://www.cdc.gov/niosh/idlh/64186.html |title = Formic acid |work = Immediately Dangerous to Life or Health Concentrations (IDLH) |publisher = National Institute for Occupational Safety and Health |date = 4 December 2014 |accessdate = 26 March 2015}}</ref>
| PEL = TWA 5 ppm (9 mg/m<sup>3</sup>)<ref name=PGCH>{{PGCH|0296}}</ref>
| IDLH = 30 ppm<ref name=PGCH/>
| REL = TWA 5 ppm (9 mg/m<sup>3</sup>)<ref name=PGCH/>
| LC50 = 7853 ppm (rat, 15 min)<br/>3246 ppm (mouse, 15 min)<ref name=IDLH/>
 }}
|Section8={{Chembox Related
| OtherFunction_label = [[carboxylic acid]]s
| OtherFunction = [[Acetic acid]]<br/>[[Propionic acid]]
| OtherCompounds = [[Formaldehyde]]<br/>[[Methanol]]}}
}}
[[File:Formica_rufa_Quadrat.jpg|thumb|Formic acid is named after the ants that use it for attack and defense]]
'''Formic acid''', or ''' methanoic acid''', is the simplist [[carboxylic acid]] and has the [[chemical formula]] {{chem|[[Hydrogen|H]]|[[Carbon|C]]|[[Oxygen|O]]|2|H}}. Many [[Animal|animals]] use for [[defence]]. The word "formic" comes from the Latin word for [[ant]], formica, referring to its early isolation by the distillation of ant bodies, and the trivial name in some languages means "ant-acid", such as Dutch mierenzuur, Danish myresyre, Faroese meyrusýra, Français acide formique and German Ameisensäure. Esters, salts, and the anions derived from formic acid are called formates.

In the 15th century, many [[alchemist]]s reported that [[ant]]s use an acidid fluid for defense. English naturalist [[John Ray]] was the first to get formic acid, by [[distillation|distilling]] ants, in 1671. 

In nature, it is found in most ants.<ref>Hoffman, Donald R. "Ant venoms" ''Current Opinion in Allergy and Clinical Immunology'' 2010, vol. 10, pages 342–346. {{doi|10.1097/ACI.0b013e328339f325}}</ref> The wood ants from the genus [[Formica]] can spray formic acid on their preys or to defend the nest. It is also known from the trichomes of [[stinging nettle]] (''Urtica dioica''). Formic acid is a naturally occurring component of the atmosphere due primarily to forest emissions.<ref>{{cite journal |journal= Geophysical Research Letters |authors= Sanhueza, E., & Andreae, M. O. |year= 1991 |title= Emission of formic and acetic acids from tropical savanna soils. |volume = 18 |issue = 9 |pages= 1707–1710|doi= 10.1029/91GL01565 |bibcode= 1991GeoRL..18.1707S }}</ref>

==References==
{{Reflist}}

[[Category:Ants]]
[[Category:Carboxylic acids|1]]