Dimethyl sulfate

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Dimethyl sulfate
Dimethylsulfate.png
Dimethyl sulfate -Molecule-3D-balls-by-AHRLS-2012.png
Names
Other names
Sulfuric acid dimethyl ester; Me2SO4; DMSO4; Dimethyl ester of sulfuric acid, Methyl sulfate
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.963
KEGG
Properties
C2H6O4S
Molar mass 126.13 g/mol
Appearance Colorless, oily liquid
Odor faint, onion-like[1]
Density 1.33 g/ml, liquid
Melting point −32 °C (−26 °F; 241 K)
Boiling point 188 °C (370 °F; 461 K) (decomposes)
Reacts
Solubility Methanol, dichloromethane, acetone
Vapor pressure 0.1 mmHg (20°C)[1]
-62.2·10−6 cm3/mol
Hazards
Main hazards Extremely toxic, contact hazard, inhalation hazard, corrosive, environmental hazard, carcinogenic, mutagenic
R-phrases (outdated) R45, R25, R26, R34,
R43, R68
S-phrases (outdated) S53, S45, S30, S60, S61
NFPA 704
Flammability code 2: Must be moderately heated or exposed to relatively high ambient temperature before ignition can occur. Flash point between 38 and 93 °C (100 and 200 °F). E.g., diesel fuelHealth code 4: Very short exposure could cause death or major residual injury. E.g., VX gasReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calciumSpecial hazards (white): no codeNFPA 704 four-colored diamond
2
4
1
Flash point 83 °C; 182 °F; 356 K [1]
Lethal dose or concentration (LD, LC):
8.6 ppm (rat, 4 hr)
75 ppm (guinea pig, 20 min)
53 ppm (mouse)
32 ppm (guinea pig, 1 hr)[2]
97 ppm (human, 10 min)[2]
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 1 ppm (5 mg/m3) [skin][1]
REL (Recommended)
Ca TWA 0.1 ppm (0.5 mg/m3) [skin][1]
IDLH (Immediate danger)
Ca [7 ppm][1]
Related compounds
Related compounds
Diethyl sulfate, methyl triflate, dimethyl carbonate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Dimethyl sulfate is a chemical compound with formula (CH3O)2SO2. As the diester of methanol and sulfuric acid, its formula is often written as (CH3)2SO4 or even Me2SO4, where CH3 or Me is methyl. Me2SO4 is mainly used as a methylating agent in organic synthesis.

Me2SO4 is a colourless oily liquid with a slight onion-like odour (although smelling it would represent significant exposure). Like all strong alkylating agents, Me2SO4 is extremely toxic. Its use as a laboratory reagent has been superseded to some extent by methyl triflate, CF3SO3CH3, the methyl ester of trifluoromethanesulfonic acid.

History[edit]

Dimethyl sulfate was discovered in the early 19th century in an impure form.[3] P. Claesson later extensively studied its preparation.[4][5] It was used in chemical warfare in WWI.[6][7]

Production[edit]

Dimethyl sulfate can be synthesized in the laboratory by many different methods,[8] the simplest being the esterification of sulfuric acid with methanol:

2 CH3OH + H2SO4 → (CH3)2SO4 + 2 H2O

Another possible synthesis involves distillation of methyl hydrogen sulfate:[5]

2 CH3HSO4 → H2SO4 + (CH3)2SO4

Methyl nitrite and methyl chlorosulfonate also result in dimethyl sulfate:[5]

CH3ONO + (CH3)OSO2Cl → (CH3)2SO4 + NOCl

Me2SO4 has been produced commercially since the 1920s. A common process is the continuous reaction of dimethyl ether with sulfur trioxide.[9]

(CH3)2O + SO3 → (CH3)2SO4

Uses[edit]

Dimethyl sulfate is best known as a reagent for the methylation of phenols, amines, and thiols. One methyl group is transferred more quickly than the second. Methyl transfer is assumed to occur via an SN2 reaction. Compared to other methylating agents, dimethyl sulfate is preferred by the industry because of its low cost and high reactivity.

Methylation at oxygen[edit]

Most commonly Me2SO4 is employed to methylate phenols. Some simple alcohols are also suitably methylated, as illustrated by the conversion of tert-butanol to t-butyl methyl ether:

2 (CH3)3COH + (CH3O)2SO2 → 2 (CH3)3COCH3 + H2SO4

Alkoxide salts are rapidly methylated:[10]

RO Na+ + (CH3O)2SO2 → ROCH3 + Na(CH3)SO4

The methylation of sugars is called Haworth methylation.[11]

Methylation at amine nitrogen[edit]

Me2SO4 is used to prepare both quaternary ammonium salts or tertiary amines:

C6H5CH=NC4H9 + (CH3O)2SO2 → C6H5CH=N+(CH3)C4H9 + CH3OSO3

Quaternized fatty ammonium compounds are used as a surfactant or fabric softeners. Methylation to create a tertiary amine is illustrated as:[10]

CH3(C6H4)NH2 + (CH3O)2SO2 (in NaHCO3 aq.) → CH3(C6H4)N(CH3)2 + Na(CH3)SO4

Methylation at sulfur[edit]

Similar to the methylation of alcohols, mercaptide salts are easily methylated by Me2SO4:[10]

RSNa+ + (CH3O)2SO2 → RSCH3 + Na(CH3)SO4

An example is:[12]

p-CH3C6H4SO2Na + (CH3O)2SO2 → p-CH3C6H4SO2CH3 + Na(CH3)SO4

This method has been used to prepare thioesters:

RC(O)SH + (CH3O)2SO2 → RC(O)S(CH3) + HOSO3CH3

Reactions with nucleic acids[edit]

Dimethyl sulfate can effect the base-specific cleavage of DNA by attacking the imidazole rings present in guanine.[13] Dimethyl sulfate also methylates adenine in single-stranded portions of DNA (e.g., those with proteins like RNA polymerase progressively melting and re-annealing the DNA). Upon re-annealing, these methyl groups interfere with adenine-guanine base-pairing. Nuclease S1 can then be used to cut the DNA in single-stranded regions (anywhere with a methylated adenine). This is an important technique for analyzing protein-DNA interactions.

Alternatives[edit]

Although dimethyl sulfate is highly effective and affordable, its toxicity has encouraged the use of other methylating reagents. Methyl iodide is a reagent used for O-methylation, like dimethyl sulfate, but is less hazardous and more expensive.[12] Dimethyl carbonate, which is less reactive, has far lower toxicity compared to both dimethyl sulfate and methyl iodide.[14] High pressure can be used to accelerate methylation by dimethyl carbonate. In general, the toxicity of methylating agents is correlated with their efficiency as methyl transfer reagents.

Safety[edit]

Dimethyl sulfate is carcinogenic[9] and mutagenic, highly poisonous, corrosive, environmentally hazardous.[15] Dimethyl sulfate is absorbed through the skin, mucous membranes, and gastrointestinal tract, and can cause a fatal delayed respiratory tract reaction. An ocular reaction is also common. There is no strong odor or immediate irritation to warn of lethal concentration in the air. The LD50 (acute, oral) is 205 mg/kg (rat) and 140 mg/kg (mouse), and LC50 (acute) is 45 ppm / 4 hours (rat).[16] The vapor pressure of 65 Pa[17] is sufficiently large to produce a lethal concentration in air by evaporation at 20 °C. Delayed toxicity allows potentially fatal exposures to occur prior to development of any warning symptoms.[15] Symptoms may be delayed 6–24 hours. Concentrated solutions of bases (ammonia, alkalis) can be used to hydrolyze minor spills and residues on contaminated equipment, but the reaction may become violent with larger amounts of dimethyl sulfate (see ICSC). Although the compound hydrolyses, treatment with water cannot be assumed to decontaminate dimethyl sulfate.

References[edit]

  1. ^ a b c d e f "NIOSH Pocket Guide to Chemical Hazards #0229". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ a b "Dimethyl sulfate". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  3. ^ Dumas, J.; Péligot, E. (1835). "Mémoire sur l'esprit de bois et sur les divers composés ethérés qui en proviennent" [Memoir on spirit of wood [i.e., methanol] and on various ethereal compounds that come from it]. Annales de Chimie et de Physique. 2nd series (in French). 58: 5–74.
  4. ^ Claesson, Peter (1879). "Ueber die neutralen und sauren Sulfate des Methyl- und Aethylalkohols" [On the neutral and acid sulfates of methyl and ethyl alcohol]. Journal für praktische Chemie. 2nd series (in German). 19: 231–265.
  5. ^ a b c Suter, C. M. (1944). The Organic Chemistry of Sulfur: Tetracovalent Sulfur Compounds. John Wiley & Sons. pp. 49–53. LCCN 44001248.
  6. ^ "Dimethyl Sulfate 77-78-1". EPA.
  7. ^ "Poison Facts: Low Chemicals: Dimethyl Sulfate". The University of Kansas Hospital.
  8. ^ Shirley, D. A. (1966). Organic Chemistry. Holt, Rinehart and Winston. p. 253. LCCN 64010030.
  9. ^ a b "Dimethyl Sulfate CAS No. 77-78-1" (PDF). 12th Report on Carcinogens (RoC). US Department of Health and Human Services. 2011.
  10. ^ a b c Dupont product information
  11. ^ W. N. Haworth (1915). "III. A New Method of Preparing Alkylated Sugars". Journal of the Chemical Society, Transactions. 107: 8–16. doi:10.1039/CT9150700008.
  12. ^ a b Fieser, L. F.; Fieser, M. (1967). Reagents for Organic Synthesis. John Wiley & Sons. p. 295. ISBN 9780471258759.
  13. ^ Streitwieser, A.; Heathcock, C. H.; Kosower, E. M. (1992). Introduction to Organic Chemistry (4th ed.). Macmillan. p. 1169. ISBN 978-0024181701.
  14. ^ Shieh, W. C.; Dell, S.; Repic, O. (2001). "1,8-Diazabicyclo[5.4.0]undec-7-ene (DBU) and Microwave-Accelerated Green Chemistry in Methylation of Phenols, Indoles, and Benzimidazoles with Dimethyl Carbonate". Organic Letters. 3 (26): 4279–4281. doi:10.1021/ol016949n. PMID 11784197.
  15. ^ a b Rippey, J. C. R.; Stallwood, M. I. (2005). "Nine Cases of Accidental Exposure to Dimethyl Sulphate — A Potential Chemical Weapon" (pdf). Emergency Medicine Journal. 22 (12): 878–879. doi:10.1136/emj.2004.015800. PMC 1726642. PMID 16299199.
  16. ^ "Material Safety Data Sheet - Dimethyl sulfate MSDS". ScienceLab.
  17. ^ ICSC

External links[edit]