Methyl formate, also called methyl methanoate, is the methyl ester of formic acid. The simplest example of a carboxylate ester, it is a colorless liquid with an ethereal odour, high vapor pressure, and low surface tension. It is a precursor to many other compounds of commercial interest.^[4]

Quick Facts Names, Identifiers ...

Methyl formate

Names
Preferred IUPAC name Methyl formate
Systematic IUPAC name Methyl methanoate
Other names R-611
Identifiers
CAS Number	107-31-3 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:77699 Y
ChEMBL	ChEMBL295026 Y
ChemSpider	7577 Y
ECHA InfoCard	100.003.166
EC Number	209-282-1
PubChem CID	7865
UNII	1MPH591FTG Y
CompTox Dashboard (EPA)	DTXSID5025609
InChI InChI=1S/C2H4O2/c1-4-2-3/h2H,1H3 Y Key: TZIHFWKZFHZASV-UHFFFAOYSA-N Y InChI=1/C2H4O2/c1-4-2-3/h2H,1H3 Key: TZIHFWKZFHZASV-UHFFFAOYAI
SMILES O=COC
Properties
Chemical formula	C2H4O2
Molar mass	60.052 g·mol−1
Appearance	Colorless liquid
Odor	pleasant[1]
Density	0.98 g/cm3
Melting point	−100 °C (−148 °F; 173 K)
Boiling point	32 °C (90 °F; 305 K)
Solubility in water	30% (20°C)[1]
Vapor pressure	634 hPa (476 mmHg) (20°C)[1]
Magnetic susceptibility (χ)	-32.0·10−6 cm3/mol
Hazards
GHS labelling:[2]
Pictograms
Signal word	Danger
Hazard statements	H224, H302, H319, H332, H335
Precautionary statements	P210, P233, P240, P241, P242, P243, P261, P264, P270, P271, P280, P301+P312, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P312, P330, P337+P313, P370+P378, P403+P233, P403+P235, P405, P501
NFPA 704 (fire diamond)	2 4 0
Flash point	−19 °C; −2 °F; 254 K[1]
Explosive limits	4.5%-23%[1]
Lethal dose or concentration (LD, LC):
LD50 (median dose)	1622 mg/kg (oral, rabbit)[3]
LCLo (lowest published)	50,000 ppm (guinea pig, 20 min)[3]
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 100 ppm (250 mg/m3)[1]
REL (Recommended)	TWA 100 ppm (250 mg/m3) ST 150 ppm (375 mg/m3)[1]
IDLH (Immediate danger)	4500 ppm[1]
Safety data sheet (SDS)	Oxford MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

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In the laboratory, methyl formate can be produced by the condensation reaction of methanol and formic acid, as follows:

HCOOH + CH₃OH → HCOOCH₃ + H₂O

Industrial methyl formate, however, is usually produced by the combination of methanol and carbon monoxide (carbonylation) in the presence of a strong base, such as sodium methoxide:^[4]

This process, practiced commercially by BASF among other companies gives 96% selectivity toward methyl formate. The catalyst for this process is sensitive to water, which can be present in the carbon monoxide feedstock, which is commonly derived from synthesis gas. Very dry carbon monoxide is, therefore, essential.^[5]

Methyl formate is used primarily to manufacture formamide, dimethylformamide, and formic acid. These compounds are precursors or building blocks for many useful derivatives.

Because of its high vapor pressure, it is used for quick-drying finishes and as a blowing agent for some polyurethane foam applications (for example Ecomate® manufactured by Foam Supplies Inc.) and as a replacement for CFCs, HCFCs, and HFCs. Methyl formate has zero ozone depletion potential and zero global warming potential^{[citation needed]}. It is also used as an insecticide.

A historical use of methyl formate, which sometimes brings it attention, was in refrigeration. Before the introduction of less-toxic refrigerants, methyl formate was used as an alternative to sulfur dioxide in domestic refrigerators, such as some models of the famous GE Monitor Top.