Pure aspirin as a fluffy, crystalline powder
| Other names
|Molar mass||180.157 g/mol|
|Melting point||135 °C (275 °F; 408 K)|
|Boiling point||140 °C (284 °F; 413 K) (decomposes)|
|0.3 g/100 ml (20 °C)|
|Solubility||Soluble in alcohols|
|Solubility in chloroform||6 g/100 ml|
|Solubility in diethyl ether||10 g/100 ml|
|Solubility in ethanol||20 g/100 ml|
|Vapor pressure||~0 mmHg|
|Safety data sheet||Sigma-Aldrich|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Acetylsalicylic acid or 2-(acetoxy)benzoic acid, is an organic acid commonly known as aspirin.
Acetylsalicylic acid (ASA) is prone to hydrolysis, breaking down into salicylic acid and acetic acid. Solutions of ASA are therefore not very stable and hot or boiling water will quickly break apart the molecule into the two smaller organic acids. The solid must be protected from air as moisture in the air will also degrade it.
Hydrolysis of ASA can be observed through the smell of acetic acid, solutions that have undergone significant hydrolysis have a very noticeable vinegar smell to them.
Acetylsalicylic acid readily hydrolyzes in hot water or solutions that are highly acidic or basic. While this can be an obstacle for some syntheses, it can be taken advantage of to make the more stable salicylic acid, which fills many of the same roles, by refluxing acetylsalicylic acid powder in low pH solution, cooling, and filtering out the crystals of salicylic acid, which should be recrystallized.
ASA reacts with sodium carbonate and bicarbonate to form sodium acetylsalicylate. Sodium hydroxide cannot be used to make the sodium salt as it will hydrolyze the ASA.
Purified aspirin is the precursor in one of the most commonly used syntheses of trinitrophenol (picric acid), a dye and explosive.
'Copper aspirinate' can be formed by using the ASA as a ligand to the copper(II) ions, or simply precipitated by the mixture of solutions of copper(II) sulfate and sodium acetylsalicylate. This is discussed in detail at http://www.sciencemadness.org/talk/viewthread.php?tid=9920
As one of the world's most commonly used medicine, aspirin is found in every pharmacy on earth as well as most supermarkets. Even basic aspirin tablets contain some form of binder to keep it in tablet form or make it more air stable. To remove these, the tablets can be crushed and washed with denatured alcohol. The ASA is soluble in the alcohol while the binders are not, so any solids that remain undissolved can be filtered off.
The alcohol can then be carefully boiled off or evaporated away. Acetylsalicylic acid forms light, fluffy, glittering white crystals when recrystallized from solution. These crystals should be stored in a dry, airtight container to prevent hydrolysis. Some hydrolysis to salicylic acid and acetic acid is unavoidable, however, so acetylsalicylic acid cannot be kept for very long periods of time in open air without loss in purity.
Acetylsalicylic acid is prepared via the esterification of salicylic acid with acetic anhydride. This reaction is performed in the presence of a small amount of catalyst, such as sulfuric acid or phosphoric acid. The reaction yields aspirin and acetic acid. The acetic acid is neutralized and the aspirin is extracted.
- Make sodium acetylsalicylate
- Picric acid synthesis
- Copper(II) acetylsalicylate synthesis
Aspirin should not be consumed in large quantities, as it has anticoagulant properties and can cause gastrointestinal bleeding. Lab grade aspirin should never be consumed.
Aspirin should be kept in a dry place to prevent hydrolysis.
Aspirin can be safely poured down the drain on dumped in the trash.