Methyl bisulfate

Methyl bisulfate
Skeletal formula
Ball-and-stick model
Names
Other names
Methyl sulfate; Methylsulfuric acid; Methyl hydrogen sulfate; Monomethyl sulfate; Metilsulfate
Identifiers
75-93-4 YesY
3D model (Jmol) Interactive image
ChEBI CHEBI:17760 N
ChemSpider 6172 N
ECHA InfoCard 100.000.834
EC Number 201-058-1
KEGG C00200 N
PubChem 6412
Properties
CH4O4S
Molar mass 112.10 g·mol−1
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

Methyl bisulfate is a chemical compound with the molecular formula CH4O4S. This compound is the mono-methyl ester of sulfuric acid. The significance of methyl bisulfate is that it is an intermediate in the hydrolysis of the important reagent dimethyl sulfate, (CH3)2SO4:[1]

(CH3)2SO4 + H2O → (CH3)HSO4 + CH3OH

Methyl bisulfate is an acid:

(CH3)HSO4 → (CH3)SO4− + H+

Methyl bisulfate came into the public view in 1993 with the discovery that certain mercury compounds catalyze the conversion of methane to methylbisulfate in good yields with excellent selectivity in concentrated sulfuric acid.[2] However, because of the toxicity and concerns with the use of mercury it wasn't until 1998 when platinum complexes were found that catalyze the reaction of CH4 by SO3 and O2 that it came into the limelight:[3][4][5]

CH4 + SO3 + 1/2 O2 → (CH3)HSO4

This discovery pointed to a possible method for upgrading inexpensive and abundantly available methane (natural gas) into methanol, which is both a more useful chemical and more easily shipped than methane. The process is proposed to proceed via an intermediate containing the Pt-CH3 group.[6]

Methyl bisulfate is used as a counterion in the formulation of some pharmaceutical drugs, where is is typically referred to as metilsulfate.[7]

References

  1. ↑ Robertson, R. E.; Sugamon, S.E. (1966). "The Hydrolysis of Dimethyl Sulfate and Diethyl Sulfate in Water". Canadian Journal of Chemistry. 44 (14): 1728–1730. doi:10.1139/v66-260.
  2. ↑ Periana, R.A.; Taube, D.J.; Evitt, E.R.; Loffler, D.G.; Wentrcek, P.R.; Voss, G.; Masuda, T. (1993). "A Mercury-Catalyzed, High-Yield System for the Oxidation of Methane to Methanol". Science. 259 (5093): 340–343. doi:10.1126/SCIENCE.259.5093.340. PMID 17832346.
  3. ↑ Hristov, I. H.; Ziegler, T. (2003). "The Possible Role of SO3 as an Oxidizing Agent in Methane Functionalization by the Catalytica Process. A Density Functional Theory Study". Organometallics. 22 (8): 1668–1674. doi:10.1021/om020774j.
  4. ↑ Periana, R. A.; Mirinov, O.; Taube, D. J.; Gamble, S (2002). "High Yield Conversion of Methane to Methyl Bisulfate Catalyzed by Iodine Cations". Chemical Communications (20): 2376–2377. doi:10.1039/b205366g.
  5. ↑ Wolf, D. (1999). "High Yields of Methanol from Methane by C-H Bond Activation at Low Temperatures". Angewandte Chemie International Edition. 37 (24): 3351–3353. doi:10.1002/(SICI)1521-3773(19981231)37:24<3351::AID-ANIE3351>3.0.CO;2-U.
  6. ↑ Periana, R. A.; Taube, D. J.; Gamble, S.; Taube, H.; Satoh, T.; Fujii, H. (1998). "Platinum Catalysts for the High-Yield Oxidation of Methane to a Methanol Derivative". Science. 280 (5363): 560–564. doi:10.1126/science.280.5363.560. PMID 9554841.
  7. ↑ International nonproprietary names (INN) for pharmaceutical substances. World Health Organization.
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