Hair-like crystals of salicylic acid in the bottom of a beaker. (Click to see up close)
| IUPAC name
| Other names
|Molar mass||138.12 g/mol|
|Appearance||Colorless crystalline solid|
|Density||1.443 g/cm3 (20 °C)|
|Melting point||158.6 °C (317.5 °F; 431.8 K)|
|Boiling point||200 °C (392 °F; 473 K) (decomposes)|
| 0.124 g/100 ml (0 °C)|
0.248 g/100 ml (25 °C)
0.414 g/100 ml (40 °C)
1.741 g/100 ml (75 °C)
7.779 g/100 ml (100 °C)
|Solubility|| Soluble in acetone, chloroform, diethyl ether, ethanol, methanol, propanol, oil of turpentine|
Slightly soluble in benzene, CCl4, toluene
|Solubility in acetone||39.6 g/100 g (23 °C)|
|Solubility in benzene|| 0.46 g/100 g (11.7 °C)|
0.775 g/100 g (25 °C)
0.991 g/100 g (30.5 °C)
2.38 g/100 g (49.4 °C)
4.4 g/100 g (64.2 °C)
|Solubility in chloroform|| 2.22 g/100 ml (25 °C)|
2.31 g/100 ml (30.5 °C)
|Solubility in methanol|| 40.67 g/100 g (−3 °C)|
62.48 g/100 g (21 °C)
|Solubility in olive oil||2.43 g/100 g (23 °C)|
|Vapor pressure||8.2·10-5 mmHg (25 °C)|
|Acidity (pKa)|| 1 = 2.97 (25 °C)|
2 = 13.82 (20 °C)
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
|Flash point||157 °C (315 °F; 430 K) (closed cup)|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|480 mg/kg (mice, oral)|
| Acetylsalicylic acid|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Salicylic acid is the organic compound with the chemical formula C6H4(OH)COOH. It is an example of a phenolic acid. It is the active metabolite of aspirin and is also used in many other medications such as skin-care products.
Decarboxylation of salicylic acid via heating will yield phenol.
- C6H4(OH)COOH → C6H5OH + CO2
Esterification with acetic anhydride gives aspirin.
- C6H4(OH)COOH + (CH3O)2O → C6H4(CH3OCO)COOH + CH3COOH
Salicylic acid is most often encountered as a fine, fluffy crystalline powder or as needle-like crystals which are difficult to compact. It has a somewhat minty and irritating odor. Salicylic acid is quite soluble in alcohols, acetone, diethyl ether, and slightly lower in nonpolar solvents, such as benzene and toluene, has low solubility in cold to warm water, and high solubility in boiling water.
Salicylic acid, while usually produced using aspirin as a precursor with ease, can also be purchased in solution as various skin-care products for treating warts or acne, those these can be both expensive and impure, as well as highly diluted.
It can also be found in food stores as preservative, usually as a ester or salt, or sometimes as free acid. Sodium salicylate is more commonly available. The obtain the free acid, simply add a stronger acid to the sodium salt and purify the compound.
Salicylic acid can be extracted from willow tree bark, by boiling said bark in water, precipitate the impurities, filter, then hydrolyze the resulting salicin to obtain crude salicylic acid. The crude salicylic acid is dissolved in hot water and recrystallized from the solution. Repeated recrystallizations may be needed to remove impurities, namely tannins. This is how salicylic acid was historically prepared.
Salicylic acid can be easily synthesized using either methyl salicylate or acetylsalicylic acid (aspirin) as the primary precursor, but because methyl salicylate may not be as cheaply or easily obtained as aspirin, it is usually synthesized from the latter, which is also typically seen as the easier process.
Production from aspirin requires the acetylsalicylic acid to be refluxed in the presence of a stronger acid (often hydrochloric acid) for a period of time, hydrolyzing it to salicylic acid and acetic acid. The product can then be washed and recrystallized.
- Make aspirin
- Make Pepto-Bismol (bismuth subsalicylate)
- Esterification of salicylic acid with methanol to make methyl salicylate
- Reaction of salicylic acid with carbamide and boric acid to form Salicylamide
- Make phenol
- Make Salsalate
- Skin exfoliation
Salicylic acid has the ability to break down lipids in the skin, causing symptoms ranging from dryness and irritation at low concentrations to mild acid burns at higher ones. When ingested orally in large amounts it can cause salicylate intoxication, which may produce very serious side effects.
No special storage is required, salicylic acid can be stored in any clean container, plastic or glass.
Salicylic acid can be safely poured down the drain or dumped in the trash, as it does not pose any danger for the environment.
A reflux setup for producing salicylic acid by Alexleyenda's process.
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