Dehydration reaction

In chemistry, a dehydration reaction is a chemical reaction that involves the loss of water from the reacting molecule or ion. Dehydration reactions are common processes, the reverse of a hydration reaction.

Dehydration reactions in organic chemistryEdit


The classic example of a dehydration reaction is the Fischer esterification, which involves treating a carboxylic acid with an alcohol to give an ester:

RCO2H + R′OH ⇌ RCO2R′ + H2O

Often such reactions require the presence of a dehydrating agent, i.e. a substance that reacts with water.


Two monosaccharides, such as glucose and fructose, can be joined together (to form saccharose) using dehydration synthesis. The new molecule, consisting of two monosaccharides, is called a disaccharide.

Nitrile formationEdit

Nitriles are often prepared by dehydration of primary amides.

RC(O)NH2 → RCN + H2O

Ketene formationEdit

Ketene is produced by heating acetic acid and trapping the product:[1]

CH3CO2H → CH2=C=O + H2O

Alkene formationEdit

Alkenes can be made from alcohols by dehydration. This conversion, among others, is a key reaction in converting biomass to liquid fuels.[2] The conversion of ethanol to ethene is a fundamental example:[3][4]

   CH3CH2OH → H2C=CH2 + H2O

The reaction is slow in the absence of an acid catalysts such as sulfuric acid and certain zeolites.

Some alcohols are prone to dehydration. 3-Hydroxylcarbonyls, called aldols, release water upon standing at room temperature:


In the dienol benzene rearrangement, dehydration leads to aromatization.[5][6]

Often the reaction is induced by dehydrating reagents. For example, 2-methyl-cyclohexan-1-ol dehydrates to 1-methylcyclohexene in the presence of Martin's sulfurane, which reacts irreversibly with water.[7][8]


Double dehydration is illustrated by the conversion of glycerol to acrolein:[9][10]


Dehydration reactions in inorganic chemistryEdit

The formation of the pyrophosphate bond is an important dehydration relevant to bioenergetics.

Various construction materials are produced by dehydration. Plaster of Paris is produced by dehydration of gypsum in a kiln:,[11][12]

  heat     (released as steam).

The resulting dry powder is ready to be mixed with water to form a stiff but workable paste that hardens.

See alsoEdit


  1. ^ Miller, Raimund; Abaecherli, Claudio; Said, Adel; Jackson, Barry (2001). "Ketenes". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_063.
  2. ^ . doi:10.1021/cr4002269. Cite journal requires |journal= (help); Missing or empty |title= (help)
  3. ^ Zimmermann, Heinz; Walz, Roland (2008). "Ethylene". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a10_045.pub3. ISBN 978-3527306732.
  4. ^ . doi:10.1021/ie401157c. Cite journal requires |journal= (help); Missing or empty |title= (help)
  5. ^ H. Plieninger; Gunda Keilich (1956). "Die Dienol-Benzol-Umlagerung" [The dienol-benzene rearrangement]. Angew. Chem. (in German). 68 (19): 618. doi:10.1002/ange.19560681914.
  6. ^ Margaret Jevnik Gentles; Jane B. Moss; Hershel L. Herzog; E. B. Hershberg (1958). "The Dienol-Benzene Rearrangement. Some Chemistry of 1,4-Androstadiene-3,17-dione". J. Am. Chem. Soc. 80 (14): 3702–3705. doi:10.1021/ja01547a058.
  7. ^ J. Brent Friesen; Robert Schretzman (2011). "Dehydration of 2-Methyl-1-cyclohexanol: New Findings from a Popular Undergraduate Laboratory Experiment". J. Chem. Educ. 88 (8): 1141–1147. Bibcode:2011JChEd..88.1141F. doi:10.1021/ed900049b.
  8. ^ Roden, Brian A. (2001). "Diphenylbis(1,1,1,3,3,3-hexafluoro-2-phenyl-2-propoxy)sulfurane". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rd409. ISBN 0471936235.
  9. ^ H. Adkins; W. H. Hartung (1926). "Acrolein". Organic Syntheses. 6: 1. doi:10.15227/orgsyn.006.0001.
  10. ^ . doi:10.1039/c0gc00307g. Cite journal requires |journal= (help); Missing or empty |title= (help)
  11. ^ Franz Wirsching "Calcium Sulfate" in Ullmann's Encyclopedia of Industrial Chemistry, 2012 Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_555
  12. ^ Staff. "CaSO4, ½ H2O". LaFargePrestia. Archived from the original on November 20, 2008. Retrieved 27 November 2008.