Potassium methoxide

From Wikipedia, the free encyclopedia
Methanolat-Ion.svg  K+.svg
Methoxide-3D-vdW.png
Potassium-3D.png
Names
IUPAC name
Potassium methoxide
Systematic IUPAC name
Potassium methylate
Identifiers
  • 865-33-8 (hydrogen error) ☒N
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.011.579 Edit this at Wikidata
EC Number
  • 212-736-1
UNII
UN number 3206
  • InChI=1S/CH3O.K/c1-2;/h1H3;/q-1;+1
    Key: BDAWXSQJJCIFIK-UHFFFAOYSA-N
  • InChI=1/CH3O.K/c1-2;/h1H3;/q-1;+1
    Key: BDAWXSQJJCIFIK-UHFFFAOYAD
  • [K+].[O-]C
Properties
CH3KO
Molar mass 70.132
Hazards
GHS pictograms GHS02: FlammableGHS05: CorrosiveGHS07: Harmful
GHS Signal word Danger
GHS hazard statements
 H228, H251, H290, H302, H314, H318
P210, P234, P235+410, P240, P241, P260, P264, P270, P280, P301+312, P301+330+331, P303+361+353, P304+340, P305+351+338, P310, P321, P330, P363, P370+378, P390, P404, P405, P407, P413, P420
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Potassium methoxide is the alkoxide of methanol with the counterion potassium and is used as a strong base and as a catalyst for transesterification, in particular for the production of biodiesel.

Preparation[]

The preparation of potassium methoxide can be achieved on the laboratory scale by the (strongly exothermic) reaction of metallic potassium and methanol upon the release of equimolar amounts of hydrogen.[1]

Kaliummethanolat aus Kalium und Methanol

The reaction of metal hydrides (potassium hydride) with methanol forming potassium methoxide is also possible but less important.

Kaliummethanolat aus Kaliumhydrid und Methanol

The exothermic reaction of potassium hydroxide with methanol leads in an equilibrium reaction to potassium methanolate and water (avoiding formation of highly inflammable hydrogen gas). In a continuous process the formed water must be removed permanently.[2]

Kaliummethanolat aus Kaliumhydroxid und Methanol

The complete removal of the water is critical for the reaction conversion, due to the pronounced hygroscopy of potassium hydroxide, which contains about 10% of water.[3] The significantly higher dissolution rate of potassium hydroxide in methanol compared to sodium hydroxide is advantageous.

On a large scale, potassium methoxide is produced by decomposing potassium amalgam with methanol, which is produced by the chloralkali-electrolysis of potassium chloride by the amalgam process. Impurities of the resulting potassium methoxide in methanol with metallic mercury can be eliminated by ultrafiltration.[4] Solid potassium methoxide is obtained by distilling off the methanol. Because of their simpler production and better handling for chemical purposes solutions of potassium methanolate ( 25 to 32% by weight) are preferably used, which were continuously withdrawn from the amalgam process.

The displacement of the amalgam process by the ecologically and economically superior membrane process for the preparation of the mass chemicals sodium hydroxide and potassium hydroxide will make this standard production process for the production of alkali metal alkoxides in future useless.[5]

Properties[]

Potassium methoxide is a white to yellowish, hygroscopic, odorless crystalline powder which reacts violently with water forming potassium hydroxide and methanol. The aqueous solutions obtained are highly basic and have a corrosive effect. The substance is classified as an inflammable solid with a spontaneous ignition temperature of 70 °C.[6]

The human toxicity and ecotoxicity evaluation of potassium methoxide is based on the properties of the decomposition products potassium hydroxide and methanol during hydrolysis in the aqueous medium.[citation needed]

Use[]

The carbonylation of methanol with carbon monoxide to methyl formate (methyl methanoate) is catalyzed by strong bases, such as potassium methoxide.[7][8]

The main application of potassium methoxide is use as basic transesterification catalyst in biodiesel synthesis (as a 25-32% methanolic solution). Triglycerides of vegetable and animal origin are reacted with methanol in the presence of alkali metal methanolates to form the corresponding fatty methyl esters.[9][3]

Potassium methoxide allows a facilitated formation of fatty soaps in comparison to the (lower-priced) sodium methoxide (here potassium salts of the fatty acids from the triglycerides) and higher yields are obtained with potassium methoxide. The optimum conditions for biodiesel production from canola oil are reported as being 1.59% by weight of potassium methoxide, a reaction temperature of 50 °C and a methanol/oil ratio of 4.5: 1. The biodiesel yield is 95.8% with a fatty acid content of 0.75% by weight.[10]

Literature[]

  • N.Y. Turova; E.P. Turevskaya; V.G. Kessler; M.I. Yanovskaya, eds. (2002), The Chemistry of Metal Alkoxides, Springer US, doi:10.1007/b113856, ISBN 978-0-7923-7521-0

References[]

  1. ^ A.R. Ronzio; W.B. Cook. "4-Amino-2,6-dimethylpyrimidine". Organic Syntheses. 24. doi:10.15227/orgsyn.024.0006.
  2. ^ Chimtek Engineering: Potassium Methylate Production Technology, abgerufen am 12. August 2015.
  3. ^ a b J. Ruwwe (2008), "Metal alkoxides as catalysts for the biodiesel production" (PDF), Chim. Oggi Chem. Today, 26 (1), pp. 26–28
  4. ^ EP 2656905, M. Horn, B. Helpap, M. Thiel, M. Neumann, "Entquickung von Lösungen durch Ultrafiltration" 
  5. ^ ICF International: Study on EU Implementation of the Minamata Convention on Mercury, abgerufen am 12. August 2015.
  6. ^ Evonik Industries, GPS Safety Summary, Potassium Methylate, abgerufen am 12. August 2015.
  7. ^ B.N. Pattanaik (2013), "The advances in processes and catalysts for the production of methyl formate by methanol carbonylation – a review", IJCPT, 3 (2), pp. 55–70, ISSN 2277-4807
  8. ^ US 20140148614, D. Schneider, K.-D. Mohl, M. Schäfer, J. Paschold, J.H. Teles, S. Rittinger, "Process for preparing methyl formate by reaction of methanol with carbon monoxide in the presence of a catalyst system comprising alkali metal formate and alkali metal alkoxide" 
  9. ^ G. Knothe; J. Krahl; J. Van Gerpen, eds. (2010), The Biodiesel Handbook (2nd ed.), AOCS Press, ISBN 978-1-893997-62-2
  10. ^ A. Singh; B. He; J. Thompson; J. Van Gerpen (2006), "Process optimization of biodiesel production using alkaline catalysts" (PDF), Appl. Eng. Agric., 22 (4), pp. 597–600, archived from the original (PDF) on 2015-11-23, retrieved 2017-02-13

See also[]

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