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.

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.

Nitriles are often prepared by dehydration of primary amides.

RC(O)NH₂ → RCN + H₂O

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

CH₃CO₂H → CH₂=C=O + H₂O

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

   CH₃CH₂OH → H₂C=CH₂ + H₂O

The reaction is accelerated by acid catalysts such as sulfuric acid and certain zeolites. These reactions often proceed via carbocation intermediates as shown for the dehydration of cyclohexanol.^[5]

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

RC(O)CH₂CH(OH)R' → RC(O)CH=CHR' + H₂O

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.^[6][7]

Double dehydration is illustrated by the conversion of glycerol to acrolein:^[8][9]

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:^[10][11]

${\displaystyle {\ce {CaSO4.2H2O +{}}}}$ heat ${\displaystyle {\ce {->}}}$ ${\displaystyle {\ce {CaSO4.1/2H2O + 1 1/2H2O}}}$ (released as steam).

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

• Hydration reaction
• Condensation reaction
• Hydrolysis