Carboxylic acids are organic acids characterized by the presence of one or more carboxyl groups in their molecules. A carboxyl group consists of a carbon atom attached to an oxygen atom with a double covalent bond and to a hydroxyl group by a single covalent bond. The chemical formula of the carboxyl group may be written as -C(=O)OH, -COOH, or -CO2H. Salts and anions of carboxylic acids are called carboxylates.
Carboxylic acids are widespread in nature. For example, acetic acid is present in vinegar, malic acid is found in apples, lactic acid is present in sour milk, and citric acid is contained in citrus fruits such as lemons, oranges, and grapefruits.
Lower straight-chain aliphatic carboxylic acids, as well as those of even carbon number up to C18 are commercially available. For example, acetic acid is produced by methanol carbonylation with carbon monoxide, while long chain carboxylic acids are obtained by the hydrolysis of triglycerides obtained from plant or animal oils.
The simplest series of carboxylic acids are the alkanoic acids, written as R-COOH, where R is a hydrogen atom or an alkyl group. Compounds may also have two or more carboxylic acid groups per molecule.
Carboxylic acids are polar and form hydrogen bonds with one another. At high temperatures, in the vapor phase, carboxylic acids usually exist as dimeric pairs, as shown in the diagram.
Lower carboxylic acids (containing one to four carbon atoms per molecule) are miscible with water, but higher carboxylic acids (with large alkyl groups) are much less soluble because of the increasing hydrophobic nature of the alkyl chain. They tend to be soluble in less polar solvents such as ethers and alcohols.
Carboxylic acids are Bronsted acids—that is, they are proton donors. They are typically weak acids, meaning they only partially dissociate into H+ cations and RCOO− anions in aqueous solution. For example, at room temperature, only 0.02 percent of all acetic acid molecules are dissociated in water.
Thus, in an aqueous solution, the undissociated acid exists in a chemical equilibrium with the dissociated acid:
The acidity of carboxylic acids can be explained either by the stability of the acid, or the stability of the conjugate base using inductive effects or resonance effects.
Using inductive effects, the acidity of carboxylic acids can be rationalized by the two electronegative oxygen atoms distorting the electron clouds surrounding the O-H bond, weakening it. The weak O-H bond causes the acid molecule to be less stable, and causing the hydrogen atom to be labile, thus it dissociates easily to give the H+ ion. Since the acid is unstable, the equilibrium will lie on the right.
Additional electronegative atoms or groups such as chlorine or hydroxyl, substituted on the R-group have a similar, though lesser effect. The presence of these groups increases the acidity through inductive effects. For example, trichloroacetic acid (three -Cl groups) is a stronger acid than lactic acid (one -OH group) which in turn is stronger than acetic acid (no electronegative constituent).
The acidity of a carboxylic acid can also be explained by resonance effects. The result of the dissociation of a carboxylic acid is a resonance stabilized product in which the negative charge is shared (delocalized) between the two oxygen atoms. Each of the carbon-oxygen bonds has what is called a partial double bond characteristic. Since the conjugate base is stabilized, the above equilibrium lies on the right.
Carboxylic acids can be synthesized by any of several methods. Some examples follow.
A carboxylic acid reacts with a base to form a carboxylate salt in which the hydrogen of the carboxyl group is replaced with a metal cation. For instance, acetic acid reacts with sodium hydroxide (a base) to produce sodium acetate, a water-soluble salt, and water. The reaction may be written as:
When baking soda is added to vinegar, we observe that the solution fizzes. This is because acetic acid in the vinegar reacts with baking soda (sodium bicarbonate) to produce sodium acetate, carbon dioxide (which bubbles up to create the fizz), and water. The reaction may be written as follows:
Formation of esters and amides:
Carboxylic acids also react with alcohols to give esters and with amines to generate amides. Like other alcohols and phenols, the hydroxyl group on carboxylic acids may be replaced with a chlorine atom using thionyl chloride to give acyl chlorides.
Reduction to alcohols:
Carboxylic acids may be reduced by lithium aluminum hydride or borane to give primary alcohols. It is easier, however, to reduce an ester to an alcohol.
In IUPAC nomenclature, carboxylic acids have an -oic acid suffix—for example, octadecanoic acid. In common nomenclature, the suffix is usually -ic acid—for example, stearic acid.
The carboxylate anion R-COO– is usually named with the suffix -ate. Thus, for example, the anion of acetic acid is called the acetate ion.
|Carbon atoms||Common name||IUPAC name||Chemical formula||Common location or use|
|1||Formic acid||Methanoic acid||HCOOH||Insect stings|
|2||Acetic acid||Ethanoic acid||CH3COOH||Vinegar|
|3||Propionic acid||Propanoic acid||CH3CH2COOH|
|4||Butyric acid||Butanoic acid||CH3(CH2)2COOH||Rancid butter|
|5||Valeric acid||Pentanoic acid||CH3(CH2)3COOH|
|6||Caproic acid||Hexanoic acid||CH3(CH2)4COOH|
|7||Enanthic acid||Heptanoic acid||CH3(CH2)5COOH|
|8||Caprylic acid||Octanoic acid||CH3(CH2)6COOH|
|9||Pelargonic acid||Nonanoic acid||CH3(CH2)7COOH|
|10||Capric acid||Decanoic acid||CH3(CH2)8COOH|
|12||Lauric acid||Dodecanoic acid||CH3(CH2)10COOH||Coconut oil|
|18||Stearic acid||Octadecanoic acid||CH3(CH2)16COOH|
Other carboxylic acids include:
|Chemical class: Alcohol • Aldehyde • Alkane • Alkene • Alkyne • Amide • Amine • Azo compound • Benzene derivative • Carboxylic acid • Cyanate • Ester • Ether • Haloalkane • Imine • Isocyanide • Isocyanate • Ketone • Nitrile • Nitro compound • Nitroso compound • Peroxide • Phosphoric acid • Pyridine derivative • Sulfone • Sulfonic acid • Sulfoxide • Thioether • Thiol • Toluene derivative|
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