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MAKING PHENYLAMINE This page looks in outline at the preparation of phenylamine (also known as aniline or aminobenzene) starting from benzene. The benzene is first converted to nitrobenzene which is in turn reduced to phenylamine. Benzene to nitrobenzene Benzene is nitrated by replacing one of the hydrogen atoms on the benzene ring by a nitro group, NO2. The benzene is treated with a mixture of concentrated nitric acid and concentrated sulphuric acid at a temperature not exceeding 50°C. The mixture is held at this temperature for about half an hour. Yellow oily nitrobenzene is formed.
You could write this in a more condensed form as:
The concentrated sulphuric acid is acting as a catalyst and so isn't written into the equations. The temperature is kept relatively low to prevent more than one nitro group being substituted onto the ring. | ||
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Note: Follow this link if you want the mechanism for the nitration of benzene. Use the BACK button (or the HISTORY file or GO menu) on your browser to return to this page later. | ||
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Nitrobenzene to phenylamine The conversion is done in two main stages: Stage 1: conversion of nitrobenzene into phenylammonium ions Nitrobenzene is reduced to phenylammonium ions using a mixture of tin and concentrated hydrochloric acid. The mixture is heated under reflux in a boiling water bath for about half an hour. Under the acidic conditions, rather than getting phenylamine directly, you instead get phenylammonium ions formed. The lone pair on the nitrogen in the phenylamine picks up a hydrogen ion from the acid. The electron-half-equation for this reaction is:
The nitrobenzene has been reduced by gaining electrons in the presence of the acid. The electrons come from the tin, which forms both tin(II) and tin(IV) ions.
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Note: I have given these as electron-half-equations rather than attempting full equations in order to try to show what is happening. Combining them into full equations leads you to some really scary equations where it is difficult to see what is going on. The problem is made much worse because the tin ions formed go on to react with chloride ions from the hydrochloric acid to form complex ions such as [SnCl6]2-. If you aren't sure about electron-half-equations you could follow this link - but it really isn't important for UK A level purposes to worry too much about this in the present context. You are unlikely to need much more than the conditions for the reaction. Use the BACK button on your browser to return to this page if you should decide to follow this link. | ||
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Stage 2: conversion of the phenylammonium ions into phenylamine All you need to do is to remove the hydrogen ion from the -NH3+ group. Sodium hydroxide solution is added to the product of the first stage of the reaction.
The phenylamine is formed together with a complicated mixture of tin compounds from reactions between the sodium hydroxide solution and the complex tin ions formed during the first stage. The phenylamine is finally separated from this mixture. The separation is long, tedious and potentially dangerous - involving steam distillation, solvent extraction and a final distillation. | ||
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Note: The conversion of nitrobenzene into phenylamine is so time-consuming, complicated, and hazardous at this level that I'm not going to make any attempt to describe this in detail. If you want details, refer to any good practical organic chemistry textbook. | ||
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Summary What you are likely to need for UK A level chemistry purposes can be summed up by:
You are almost bound to need the mechanism for the nitration reaction as well.
© Jim Clark 2004 (modified April 2016) |
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