Chloroform

For other uses, see Chloroform (disambiguation).

Chloroform, or Trichloromethane, is an organic compound with formula CHCl₃ and a common organic solvent. It is a colorless, strong-smelling, dense liquid produced on a large scale as a precursor to PTFE and refrigerants^[8] and is a trihalomethane that serves as a powerful anesthetic, euphoriant, anxiolytic, and sedative when inhaled or ingested. It is also part of a wider class of substances known as volatile organic compounds.^[9][10]

Chloroform

Names
Preferred IUPAC name Trichloromethane
Other names Chloroform^[1] Methane trichloride Methyl trichloride Methenyl trichloride Methenyl chloride TCM Freon 20 Refrigerant-20 R-20 UN 1888
Identifiers
CAS Number	67-66-3^Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:35255^Y
ChEMBL	ChEMBL44618^Y
ChemSpider	5977^Y
ECHA InfoCard	100.000.603
EC Number	200-663-8
KEGG	C13827^Y
PubChem CID	6212
RTECS number	FS9100000
UNII	7V31YC746X^Y
CompTox Dashboard (EPA)	DTXSID1020306
InChI InChI=1S/CHCl3/c2-1(3)4/h1H^Y Key: HEDRZPFGACZZDS-UHFFFAOYSA-N^Y InChI=1/CHCl3/c2-1(3)4/h1H Key: HEDRZPFGACZZDS-UHFFFAOYAG
SMILES ClC(Cl)Cl
Properties
Chemical formula	CHCl3
Molar mass	119.37 g·mol^−1
Appearance	Highly refractive colorless liquid
Odor	Strong smell reminiscent of dry-cleaner's shops
Density	1.564 g/cm^3 (−20 °C) 1.489 g/cm^3 (25 °C) 1.394 g/cm^3 (60 °C)
Melting point	−63.5 °C (−82.3 °F; 209.7 K)
Boiling point	61.15 °C (142.07 °F; 334.30 K) decomposes at 450 °C
Solubility in water	10.62 g/L (0 °C) 8.09 g/L (20 °C) 7.32 g/L (60 °C)
Solubility	Soluble in benzene Miscible in diethyl ether, oils, ligroin, alcohol, CCl4, CS2
Solubility in acetone	≥ 100 g/L (19 °C)
Solubility in dimethyl sulfoxide	≥ 100 g/L (19 °C)
Vapor pressure	0.62 kPa (−40 °C) 7.89 kPa (0 °C) 25.9 kPa (25 °C) 313 kPa (100 °C) 2.26 MPa (200 °C)
Henry's law constant (kH)	3.67 L·atm/mol (24 °C)
Acidity (pKa)	15.7 (20 °C)
UV-vis (λmax)	250 nm, 260 nm, 280 nm
Magnetic susceptibility (χ)	−59.30·10^−6 cm^3/mol
Thermal conductivity	0.13 W/m·K (20 °C)
Refractive index (nD)	1.4459 (20 °C)
Viscosity	0.563 cP (20 °C)
Structure
Molecular shape	Tetrahedral
Dipole moment	1.15 D
Thermochemistry
Heat capacity (C)	114.25 J/mol·K
Std molar entropy (S^⦵298)	202.9 J/mol·K
Std enthalpy of formation (ΔfH^⦵298)	−134.3 kJ/mol
Gibbs free energy (ΔfG^⦵)	−71.1 kJ/mol
Std enthalpy of combustion (ΔcH^⦵298)	473.21 kJ/mol
Pharmacology
ATC code	N01AB02 (WHO)
Hazards^[7]
Occupational safety and health (OHS/OSH):
Main hazards	Carcinogen – Reproductive toxicity – Specific target organ toxicity (STOT)^[2]^[3]^[4]
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H302, H315, H319, H331, H336, H351, H361d, H372
Precautionary statements	P201, P202, P235, P260, P264, P270, P271, P280, P281, P301+P330+P331, P302+P352, P304+P340, P305+P351+P338, P308+P313, P310, P311, P314, P332+P313, P337+P313, P362, P403+P233, P405, P501
NFPA 704 (fire diamond)	2 0 0
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	704 mg/kg (mouse, dermal)^[5]
LC50 (median concentration)	9,617 ppm (rat, 4 hr)^[6]
LCLo (lowest published)	20,000 ppm (guinea pig, 2 hr) 7,056 ppm (cat, 4 hr) 25,000 ppm (human, 5 min)^[6]
NIOSH (US health exposure limits):
PEL (Permissible)	50 ppm (240 mg/m^3)^[3]
REL (Recommended)	Ca ST 2 ppm (9.78 mg/m^3) [60-minute]^[3]
IDLH (Immediate danger)	500 ppm^[3]
Safety data sheet (SDS)	[1]
Supplementary data page
Chloroform (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is ^YN ?) Infobox references

Structure

The molecule adopts a tetrahedral molecular geometry with C_3v symmetry.^[11] The chloroform molecule can be viewed as the methane molecule with three hydrogen atoms replaced with three chlorine atoms, leaving a single hydrogen atom.

Natural occurrence

The total global flux of chloroform through the environment is approximately 660000 tonnes per year,^[12] and about 90% of emissions are natural in origin. Many kinds of seaweed produce chloroform, and fungi are believed to produce chloroform in soil.^[13] Abiotic processes are also believed to contribute to natural chloroform productions in soils although the mechanism is still unclear.^[14]

As chloroform is a volatile organic compound,^[15] it dissipates readily from soil and surface water and undergoes degradation in air to produce phosgene, dichloromethane, formyl chloride, carbon monoxide, carbon dioxide, and hydrogen chloride. Its half-life in air ranges from 55 to 620 days. Biodegradation in water and soil is slow. Chloroform does not significantly bioaccumulate in aquatic organisms.^[16]

History

Chloroform was synthesized independently by several investigators circa 1831:

• Moldenhawer, a German pharmacist from Frankfurt an der Oder, appears to have produced chloroform in 1830 by mixing chlorinated lime with ethanol; he mistook it for Chloräther (chloric ether, 1,2-dichloroethane), however.^[17][18]
• Samuel Guthrie, a U.S. physician from Sackets Harbor, New York, also appears to have produced chloroform in 1831 by reacting chlorinated lime with ethanol, as well as noting its anaesthetic properties; he also believed that he had prepared chloric ether, however.^[19][20][21]
• Justus von Liebig carried out the alkaline cleavage of chloral.^[22][23]
• Eugène Soubeiran obtained the compound by the action of chlorine bleach on both ethanol and acetone.^[24]
• In 1834, French chemist Jean-Baptiste Dumas determined chloroform's empirical formula and named it.^[25] In 1835, Dumas prepared the substance by the alkaline cleavage of trichloroacetic acid. Regnault prepared chloroform by chlorination of chloromethane.^{[citation needed]}
• In 1842, Robert Mortimer Glover in London discovered the anaesthetic qualities of chloroform on laboratory animals.^[26]
• In 1847, Scottish obstetrician James Y. Simpson was the first to demonstrate the anaesthetic properties of chloroform on humans, provided by local pharmacist William Flockhart of Duncan, Flockhart and company,^[27] and helped to popularise the drug for use in medicine.^[28] By the 1850s, chloroform was being produced on a commercial basis, in Britain about 750,000 doses a week by 1895,^[29] by using the Liebig procedure, which retained its importance until the 1960s. Today, chloroform – along with dichloromethane – is prepared exclusively and on a massive scale by the chlorination of methane and chloromethane.^[8]

Production

Industrially, chloroform is produced by heating a mixture of chlorine and either chloromethane (CH₃Cl) or methane (CH₄).^[8] At 400–500 °C, a free radical halogenation occurs, converting these precursors to progressively more chlorinated compounds:

CH₄ + Cl₂ → CH₃Cl + HCl

CH₃Cl + Cl₂ → CH₂Cl₂ + HCl

CH₂Cl₂ + Cl₂ → CHCl₃ + HCl

Chloroform undergoes further chlorination to yield carbon tetrachloride (CCl₄):

CHCl₃ + Cl₂ → CCl₄ + HCl

The output of this process is a mixture of the four chloromethanes: chloromethane, dichloromethane, trichloromethane (chloroform), and tetrachloromethane (carbon tetrachloride). This can then be separated by distillation.^[8]

Chloroform may also be produced on a small scale via the haloform reaction between acetone and sodium hypochlorite:^{[citation needed]}

3 NaClO + (CH₃)₂CO → CHCl₃ + 2 NaOH + CH₃COONa

Deuterochloroform

Main article: Deuterated chloroform

Deuterated chloroform is an isotopologue of chloroform with a single deuterium atom. CDCl₃ is a common solvent used in NMR spectroscopy. Deuterochloroform is produced by the haloform reaction,^{[citation needed]} the reaction of acetone (or ethanol) with sodium hypochlorite or calcium hypochlorite.^[8] The haloform process is now obsolete for the production of ordinary chloroform. Deuterochloroform can be prepared by the reaction of sodium deuteroxide with chloral hydrate.^[30][31]

Inadvertent formation of chloroform

The haloform reaction can also occur inadvertently in domestic settings. Bleaching with hypochlorite generates halogenated compounds in side reactions; chloroform is the main byproduct.^[32] Sodium hypochlorite solution (chlorine bleach) mixed with common household liquids such as acetone, methyl ethyl ketone, ethanol, or isopropyl alcohol can produce some chloroform, in addition to other compounds such as chloroacetone or dichloroacetone.^{[citation needed]}

Uses

In terms of scale, the most important reaction of chloroform is with hydrogen fluoride to give monochlorodifluoromethane (CFC-22), a precursor in the production of polytetrafluoroethylene (Teflon) and other fluoropolymers. :^[8]

CHCl₃ + 2HF → CHClF₂ + 2 HCl

The reaction is conducted in the presence of a catalytic amount of mixed antimony halides. Chlorodifluoromethane is then converted into tetrafluoroethylene, the main precursor to Teflon.^[33]

Solvent

The hydrogen attached to carbon in chloroform participates in hydrogen bonding.^[34][35] Worldwide, chloroform is also used in pesticide formulations, as a solvent for fats, oils, rubber, alkaloids, waxes, gutta-percha, and resins, as a cleansing agent, grain fumigant, in fire extinguishers, and in the rubber industry.^[16][36] CDCl₃ is a common solvent used in NMR spectroscopy.^{[citation needed]}

Refrigerant

Trichloromethane has been used as a precursor to make R-22 (Chlorodifluoromethane). This is done by reacting it with a solution of Hydrofluoric acid (HF) which will fluorinate the CHCl3 molecule and release hydrochloric acid as a byproduct.^[37] Prior to the enforcement of the Montreal Protocol, the majority of the trichloromethane produced in the United States, was used for the production of Chlorodifluoromethane. ^[38]

Although trichloromethane has properties such as its low boiling point and its low global warming potential of only 31 (compared to the 1,760 of R-22) which result in it having good refrigeration properties, there is little information to suggest that it has seen widespread use as a refrigerant in any consumer products.^[39]

Lewis acid

In solvents such as CCl₄ and alkanes, chloroform hydrogen bonds to a variety of Lewis bases. HCCl₃ is classified as a hard acid and the ECW model lists its acid parameters as E_A = 1.56 and C_A = 0.44.

Reagent

As a reagent, chloroform serves as a source of the dichlorocarbene :CCl₂ group.^[40] It reacts with aqueous sodium hydroxide usually in the presence of a phase transfer catalyst to produce dichlorocarbene, :CCl₂.^[41][42] This reagent effects ortho-formylation of activated aromatic rings such as phenols, producing aryl aldehydes in a reaction known as the Reimer–Tiemann reaction. Alternatively, the carbene can be trapped by an alkene to form a cyclopropane derivative. In the Kharasch addition, chloroform forms the CHCl₂ free radical in addition to alkenes.^{[citation needed]}

Anaesthetic

 

Antique bottles of chloroform

The anaesthetic qualities of chloroform were first described in 1842 in a thesis by Robert Mortimer Glover, which won the Gold Medal of the Harveian Society for that year. Glover also undertook practical experiments on dogs to prove his theories. Glover further refined his theories and presented them in the thesis for his doctorate at the University of Edinburgh in the summer of 1847. The Scottish obstetrician James Young Simpson was one of the persons required to read the thesis, but later claimed to have never read the thesis and to have come to his conclusions independently.^{[citation needed]}

On 4 November 1847, Simpson first discovered the anaesthetic qualities of chloroform on humans. He and two colleagues were entertaining themselves by trying the effects of various substances, and thus revealed the potential for chloroform in medical procedures.^[27]

A few days later, during the course of a dental procedure in Edinburgh, Francis Brodie Imlach became the first person to use chloroform on a patient in a clinical context.^[43]

In May 1848, Robert Halliday Gunning made a presentation to the Medico-Chirurgical Society of Edinburgh following a series of laboratory experiments on rabbits that confirmed Glover's findings and also refuted Simpson's claims of originality. The laboratory experiments proving the dangers of chloroform were largely ignored.^[44]

The use of chloroform during surgery expanded rapidly thereafter in Europe. In the 1850s, chloroform was used by the physician John Snow during the birth of Queen Victoria's last two children.^[45] In the United States, chloroform began to replace ether as an anesthetic at the beginning of the 20th century;^{[citation needed]} it was quickly abandoned in favor of ether upon discovery of its toxicity, however, especially its tendency to cause fatal cardiac arrhythmia analogous to what is now termed "sudden sniffer's death". Some people used chloroform as a recreational drug or to attempt suicide.^[46] One possible mechanism of action for chloroform is that it increases movement of potassium ions through certain types of potassium channels in nerve cells.^[47] Chloroform could also be mixed with other anaesthetic agents such as ether to make C.E. mixture, or ether and alcohol to make A.C.E. mixture.^{[citation needed]}

In 1848, Hannah Greener, a 15-year-old girl who was having an infected toenail removed, died after being given the anaesthetic.^[48] Her autopsy establishing the cause of death was undertaken by John Fife assisted by Robert Mortimer Glover.^[26] A number of physically fit patients died after inhaling it. In 1848, however, John Snow developed an inhaler that regulated the dosage and so successfully reduced the number of deaths.^[49]

The opponents and supporters of chloroform were mainly at odds with the question of whether the complications were solely due to respiratory disturbance or whether chloroform had a specific effect on the heart. Between 1864 and 1910, numerous commissions in Britain studied chloroform but failed to come to any clear conclusions. It was only in 1911 that Levy proved in experiments with animals that chloroform can cause cardiac fibrillation. The reservations about chloroform could not halt its soaring popularity. Between 1865 and 1920, chloroform was used in 80 to 95% of all narcoses performed in the UK and German-speaking countries. In the United States, however, there was less enthusiasm for chloroform narcosis. In Germany, the first comprehensive surveys of the fatality rate during anaesthesia were made by Gurlt between 1890 and 1897. In 1934, Killian gathered all the statistics compiled until then and found that the chances of suffering fatal complications under ether were between 1:14,000 and 1:28,000, whereas under chloroform the chances were between 1:3,000 and 1:6,000. The rise of gas anaesthesia using nitrous oxide, improved equipment for administering anaesthetics and the discovery of hexobarbital in 1932 led to the gradual decline of chloroform narcosis.^[50]

Criminal use

Chloroform has reputedly been used by criminals to knock out, daze, or even murder victims. Joseph Harris was charged in 1894 with using chloroform to rob people.^[51] Serial killer H. H. Holmes used chloroform overdoses to kill his female victims. In September 1900, chloroform was implicated in the murder of the U.S. businessman William Marsh Rice, the namesake of the institution now known as Rice University. Chloroform was deemed a factor in the alleged murder of a woman in 1991 when she was asphyxiated while sleeping.^[52] In 2002, 13-year-old Kacie Woody was sedated with chloroform when she was abducted by David Fuller and during the time that he had her, before he shot and killed her.^[53] In a 2007 plea bargain, a man confessed to using stun guns and chloroform to sexually assault minors.^[54]

Use of chloroform as an incapacitating agent has become widely recognized, bordering on clichéd, due to the popularity of crime fiction authors having criminals use chloroform-soaked rags to render victims unconscious. Nonetheless, it is nearly impossible to incapacitate someone using chloroform in this manner.^[55] It takes at least five minutes of inhaling an item soaked in chloroform to render a person unconscious. Most criminal cases involving chloroform also involve another drug being co-administered, such as alcohol or diazepam, or the victim being found to have been complicit in its administration. After a person has lost consciousness due to chloroform inhalation, a continuous volume must be administered, and the chin must be supported to keep the tongue from obstructing the airway, a difficult procedure typically requiring the skills of an anesthesiologist. In 1865 as a direct result of the criminal reputation chloroform had gained, the medical journal The Lancet offered a "permanent scientific reputation" to anyone who could demonstrate "instantaneous insensibility", i.e. losing consciousness instantaneously, using chloroform.^[56]

Safety

Exposure

Chloroform is known to form as a by-product of water chlorination along with a range of other disinfection by-products and as such is commonly present in municipal tap water and swimming pools. Reported ranges vary considerably but are generally below the current health standard for total trihalomethanes of 100μg/L.^[57] Nonetheless, the presence of chloroform in drinking water at any concentration is considered controversial by some.^{[citation needed]}

Historically, chloroform exposure may well have been higher due to its common use as an anaesthetic, as an ingredient in cough syrups, and as a constituent of tobacco smoke where DDT had previously been used as a fumigant.^[58]

Pharmacology

It is well absorbed, metabolized, and eliminated rapidly by mammals after oral, inhalation, or dermal exposure. Accidental splashing into the eyes has caused irritation.^[16] Prolonged dermal exposure can result in the development of sores as a result of defatting. Elimination is primarily through the lungs in the form of chloroform and carbon dioxide; less than 1% is excreted in the urine.^[36]

Chloroform is metabolized in the liver by the cytochrome P-450 enzymes, by oxidation to chloromethanol and by reduction to the dichloromethyl free radical. Other metabolites of chloroform include hydrochloric acid and digluathionyl dithiocarbonate, with carbon dioxide as the predominant end product of metabolism.^[59]

Like most other general anesthetics and sedative-hypnotic drugs, chloroform is a positive allosteric modulator for the GABA_A receptor.^[60] Chloroform causes depression of the central nervous system (CNS), ultimately producing deep coma and respiratory center depression.^[59] When ingested, chloroform caused symptoms similar to those seen following inhalation. Serious illness has followed ingestion of 7.5 g (0.26 oz). The mean lethal oral dose for an adult is estimated at 45 g (1.6 oz).^[16]

The anesthetic use of chloroform has been discontinued because it caused deaths due to respiratory failure and cardiac arrhythmias. Following chloroform-induced anesthesia, some patients suffered nausea, vomiting, hyperthermia, jaundice, and coma due to hepatic dysfunction. At autopsy, liver necrosis and degeneration have been observed.^[16]

Chloroform has induced liver tumors in mice and kidney tumors in mice and rats.^[16] The hepatotoxicity and nephrotoxicity of chloroform is thought to be due largely to phosgene.^[59]

Conversion to phosgene

Chloroform converts slowly in air to the extremely poisonous phosgene (COCl₂), releasing HCl in the process.^[61]

2 CHCl₃ + O₂ → 2 COCl₂ + 2 HCl

To prevent accidents, commercial chloroform is stabilized with ethanol or amylene, but samples that have been recovered or dried no longer contain any stabilizer. Amylene has been found ineffective, and the phosgene can affect analytes in samples, lipids, and nucleic acids dissolved in or extracted with chloroform.^[62] Phosgene and HCl can be removed from chloroform by washing with saturated aqueous carbonate solutions, such as sodium bicarbonate. This procedure is simple and results in harmless products. Phosgene reacts with water to form carbon dioxide and HCl,^[63] and the carbonate salt neutralizes the resulting acid.^[64]

Suspected samples can be tested for phosgene using filter paper (treated with 5% diphenylamine, 5% dimethylaminobenzaldehyde in ethanol, and then dried), which turns yellow in phosgene vapour. There are several colorimetric and fluorometric reagents for phosgene, and it can also be quantified with mass spectrometry.^[65]

Regulation

Chloroform is suspected of causing cancer (i.e., possibly carcinogenic, IARC Group 2B) as per the International Agency for Research on Cancer (IARC) Monographs. [PDF]

It is classified as an extremely hazardous substance in the United States as defined in Section 302 of the U.S. Emergency Planning and Community Right-to-Know Act (42 U.S.C. 11002), and is subject to strict reporting requirements by facilities that produce, store, or use it in significant quantities.^[66]

Bioremediation of chloroform

Some anaerobic bacteria use chloroform for their respiration, termed organohalide respiration, converting it to dichloromethane.^[67][68]

References

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    On pages 259–265, Liebig describes Chlorkohlenstoff ("carbon chloride", chloroform), but on p. 264, Liebig incorrectly states that the empirical formula of chloroform is C₂Cl₅.
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      On p. 653, Dumas states chloroform's empirical formula:

    "Es scheint mir also erweisen, dass die von mir analysirte Substance, … zur Formel hat: C₂H₂Cl₆." (Thus it seems to me to show that the substance [that was] analyzed by me … has as [its empirical] formula: C₂H₂Cl₆.) [Note: The coefficients of his empirical formula must be halved.]

    Dumas then notes that chloroform's simple empirical formula resembles that of formic acid. Furthermore, if chloroform is boiled with potassium hydroxide, one of the products is potassium formate. On p. 654, Dumas names chloroform:

    "Diess hat mich veranlasst diese Substanz mit dem Namen 'Chloroform' zu belegen." (This caused me to bestow this substance with the name "chloroform" [i.e., formyl chloride or chloride of formic acid].)

    • Reprinted in Dumas, J.-B. (1835). "Ueber die Wirkung des Chlors auf den Alkohol" [On the action of chlorine on alcohol]. Annalen der Pharmacie. 16 (2): 164–171. doi:10.1002/jlac.18350160213. from the original on 10 May 2017. Retrieved 12 May 2016.
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External links

 

Wikimedia Commons has media related to Chloroform.

• Chloroform "The Molecular Lifesaver" An article at Oxford University providing facts about chloroform.
• Concise International Chemical Assessment Document 58
• IARC Summaries & Evaluations: Vol. 1 (1972), Vol. 20 (1979), Suppl. 7 (1987), Vol. 73 (1999)
• International Chemical Safety Card 0027
• NIOSH Pocket Guide to Chemical Hazards. "#0127". National Institute for Occupational Safety and Health (NIOSH).
• NIST Standard Reference Database