This page describes the hydrolysis of amides under both acidic and alkaline conditions. It also describes the use of alkaline hydrolysis in testing for amides.

The hydrolysis of amides
What is hydrolysis?
Technically, hydrolysis is a reaction with water. That is exactly what happens when amides are hydrolysed in the presence of dilute acids such as dilute hydrochloric acid. The acid acts as a catalyst for the reaction between the amide and water.
The alkaline hydrolysis of amides actually involves reaction with hydroxide ions, but the result is similar enough that it is still classed as hydrolysis.

Hydrolysis under acidic conditions
Taking ethanamide as a typical amide:
If ethanamide is heated with a dilute acid (such as dilute hydrochloric acid), ethanoic acid is formed together with ammonium ions. So, if you were using hydrochloric acid, the final solution would contain ammonium chloride and ethanoic acid.

Note:  You might argue that because the hydrochloric acid is changed during the reaction, it isn't acting as a catalyst. In fact, it is doing two things. It is acting as a catalyst in a reaction between the amide and water which would produce ammonium ethanoate (containing ammonium ions and ethanoate ions). It is secondly reacting with those ethanoate ions to make ethanoic acid.

Hydrolysis under alkaline conditions
Again, taking ethanamide as a typical amide:
If ethanamide is heated with sodium hydroxide solution, ammonia gas is given off and you are left with a solution containing sodium ethanoate.
Using alkaline hydrolysis to test for an amide
If you add sodium hydroxide solution to an unknown organic compound, and it gives off ammonia on heating (but not immediately in the cold), then it is an amide.
You can recognise the ammonia by smell and because it turns red litmus paper blue.
The possible confusion using this test is with ammonium salts. Ammonium salts also produce ammonia with sodium hydroxide solution, but in this case there is always enough ammonia produced in the cold for the smell to be immediately obvious.

Note:  This test is OK for UK A level purposes, but there are other things which also give off ammonia on heating with sodium hydroxide solution - for example, nitriles (but you won't come across them in a practical situation at this level) and imides (but they are beyond the scope of courses at this level).


This page explains the reason for the lack of basic character in amides, and describes their dehydration to give nitriles, and their reaction with bromine and sodium hydroxide solution to form primary amines with one less carbon atom (the Hofmann degradation).

Note:  The hydrolysis of amides is described on a separate page.
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The lack of base character in amides
Unusually for compounds containing the -NH2 group, amides are neutral. This section explains why -NH2 groups are usually basic and why amides are different.
The usual basic character of the -NH2 group
Simple compounds containing an -NH2 group such as ammonia, NH3, or a primary amine like methylamine, CH3NH2, are weak bases. A primary amine is a compound where the -NH2 group is attached to a hydrocarbon group.
The active lone pair of electrons on the nitrogen atom in ammonia can combine with a hydrogen ion (a proton) from some other source - in other words it acts as a base.
With a compound like methylamine, all that has happened is that one of the hydrogen atoms attached to the nitrogen has been replaced by a methyl group. It doesn't make a huge amount of difference to the lone pair and so ammonia and methylamine behave similarly.

Note:  The reasons that these are bases and the differences between them (because there are slight differences) are explored in some detail on a page about organic bases. It would be useful to read this page before you go on because it is relevant to what is coming next.
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For example, if you dissolve these compounds in water, the nitrogen lone pair takes a hydrogen ion from a water molecule - and equilibria like these are set up:

Notice that the reactions are reversible. In both cases the positions of equilibrium lie well to the left. These compounds are weak bases because they don't hang on to the incoming hydrogen ion very well.
Both ammonia and the amines are alkaline in solution because of the presence of the hydroxide ions, and both of them turn red litmus blue.

Why doesn't something similar happen with amides?
Amides are neutral to litmus and have virtually no basic character at all - despite having the -NH2 group. Their tendency to attract hydrogen ions is so slight that it can be ignored for most purposes.

Note:  If you haven't already done so, follow the link mentioned above to the page about organic bases, and read the bit about phenylamine. It is directly relevant to what's next.
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We need to look at the bonding in the -CONH2 group.
Like any other double bond, a carbon-oxygen double bond is made up of two different parts. One electron pair is found on the line between the two nuclei - this is known as a sigma bond. The other electron pair is found above and below the plane of the molecule in a pi bond.
A pi bond is made by sideways overlap between p orbitals on the carbon and the oxygen.
In an amide, the lone pair on the nitrogen atom ends up almost parallel to these p orbitals, and overlaps with them as they form the pi bond.

The result of this is that the nitrogen lone pair becomes delocalised - in other words it is no longer found located on the nitrogen atom, but the electrons from it are spread out over the whole of that part of the molecule.
This has two effects which prevent the lone pair accepting hydrogen ions and acting as a base:
  • Because the lone pair is no longer located on a single atom as an intensely negative region of space, it isn't anything like as attractive for a nearby hydrogen ion.
  • Delocalisation makes molecules more stable. For the nitrogen to reclaim its lone pair and join to a hydrogen ion, the delocalisation would have to be broken, and that will cost energy.

Note:  If you want to look in more detail at the bonding in the carbon-oxygen double bond, you could follow this link.
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The dehydration of amides
Amides are dehydrated by heating a solid mixture of the amide and phosphorus(V) oxide, P4O10.
Water is removed from the amide group to leave a nitrile group, -CN. The liquid nitrile is collected by simple distillation.
For example, with ethanamide, you will get ethanenitrile.

Note:  This is a just a flow scheme rather than a proper equation. I haven't been able to find a single example of the use of the full equation for this reaction. In fact the phosphorus(V) oxide reacts with the water to produce mixtures of phosphorus-containing acids.

The Hofmann Degradation
The Hofmann degradation is a reaction between an amide and a mixture of bromine and sodium hydroxide solution. Heat is needed.
The net effect of the reaction is a loss of the -CO- part of the amide group. You get a primary amine with one less carbon atom than the original amide had.
The general case would be (as a flow scheme):

posted by: VEBRIA ARDINA (RSA1C110020)

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