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Dimethyl sulfate



Dimethyl sulfate
Other names Sulfuric acid, dimethyl ester; Me2SO4; DMSO4
Identifiers
CAS number 77-78-1
SMILES O=S(=O)(OC)OC
Properties
Molecular formula C2H6O4S
Molar mass 126.13 g/mol
Appearance Colorless liquid
Density 1.33 g/ml, liquid
Melting point

-32 °C

Boiling point

188 °C decomposes

Solubility in water Reacts with water
Solubility Methanol, dichloromethane, acetone
Hazards
Main hazards Poison, contact hazard, inhalation hazard, corrosive, environmental hazard, carcinogenic, mutagenic
R-phrases R45, R25, R26, R34,
R43, R68
S-phrases S53, S45
Related Compounds
Related compounds Diethyl sulfate, methyl triflate, dimethyl carbonate
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Dimethyl sulfate is a chemical compound with formula (CH3O)2SO2. As the dimethyl ester of 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.

Under standard conditions, 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 highly toxic. Its use as a laboratory reagent has been superseded to some extent by methyl triflate, CF3SO3CH3, the methyl ester of trifluoromethanesulfonic acid.

Additional recommended knowledge

Contents

History

Dimethyl sulfate was first discovered in the early 1800s in an impure form. P. Claesson later extensively studied its preparation.[1]

Production

Dimethyl sulfate can be synthesized in the laboratory by many different syntheses:[2]

2 CH3OH + H2SO4 → (CH3)2SO4 + 2 H2O

Another possible synthesis involves distillation of methyl hydrogen sulfate:[1]

2 CH3HSO4 → H2SO4 + (CH3)2SO4

Methyl nitrite and methyl chlorosulfonate also result in dimethyl sulfate[1]:

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

In the United States, Me2SO4 has been produced commercially since the 1920s. A common process is the continuous reaction of dimethyl ether with sulfur trioxide.[3]

(CH3)2O + SO3 → (CH3)2SO4

Uses

Dimethyl sulfate is best known as a reagent for the methylation of phenols, amines, and thiols. Typically, one methyl group is transferred more quickly than the second. Methyl transfer is typically assumed to occur via an SN2 reaction. 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.[4] Dimethyl carbonate has far lower toxicity compared to both dimethyl sulfate and methyl iodide and can be used to instead of dimethyl sulfate for N-methylation.[5] In general the toxicity of methylating agents is correlates with their efficiency as methyl transfer reagents.

Methylation at oxygen

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

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

Alkoxide salts are rapidly methylated:[6]

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

Methylation at amine nitrogen

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

C6H5CH=NC4C9 + (CH3O)2SO2 → C6H5CH=N+(CH3)C4C9 + CH3OSO3-

Quaternized fatty ammonium compounds are used as a surfactant or fabric softeners. The methylation of a tertiary amine is illustrated as[6]:

CH3(C6H2)NH2 + (CH3O)2SO2 (in HNCO2) → CH3(C6H2)N(CH3)2 + Na(CH3)SO4

Methylation at sulfur

Similar to the methylation of alcohols, mercaptide salts are easily methylated by Me2SO4[6]:

RS-Na+ + (CH3O)2SO2 → RSCH3 + Na(CH3)SO4

An example is:[4]

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

Other Uses

With DNA dimethyl sulfate can effect the base-specific cleavage of guanine by rupturing the imidazole rings present in guanine.[7] This process can be used to determine base sequencing, cleavage on the DNA chain, and other applications.

Safety

Dimethyl sulfate is likely carcinogenic[3] and mutagenic, poisonous, corrosive, environmentally hazardous and volatile (presenting an inhalation hazard). Some consider it a potential chemical weapon. Dimethyl sulfate is absorbed through the skin, mucous membranes, and gastrointestinal tract. Delayed toxicity allows potentially fatal exposures to occur prior to development of any warning symptoms.[8] 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 in water, plain water cannot be assumed to hydrolyze dimethyl sulfate quickly enough for decontamination purposes. The hydrolysis products, monomethyl sulfate and methanol, are environmentally hazardous. In water, the compound is ultimately hydrolyzed to sulfuric acid and methanol, which is less toxic than dimethyl sulfate.

References

  1. ^ a b c Suter, C. M. The Organic Chemistry of Sulfur Tetracovalent Sulfur Compounds John Wiley & Sons, Inc. 1944. p 49-53
  2. ^ Shirley, D. A. Organic Chemistry. Holt, Rinehart and Winston. 1966. p. 253
  3. ^ a b Substance Profiles - Dimethyl Sulfate. 11th Report on Carcinogens. Department of Health and Human Services.
  4. ^ a b Fieser, L. F. and Fieser, M. Reagents for Organic Synthesis. John Wiley & Sons, Inc. 1967. p. 295
  5. ^ W. C. Shieh, S. Dell and O. Repic (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.
  6. ^ a b c Dupont product information
  7. ^ Streitwieser, A., Heathcock, C. H., and Kosower, E. M. Introduction to Organic Chemistry. Prentice-Hall Inc. 1992. p. 1169
  8. ^ Rippey, J. and Stallwood, M. Emergency Medicine Journal 2005;22:878-879
 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Dimethyl_sulfate". A list of authors is available in Wikipedia.
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