Monoprotic acid

Monoprotic acid is a type of acid that donates only one proton or hydrogen ion per molecule to an aqueous solution. The term "monoprotic" refers to the single proton or hydrogen ion, distinguishing these acids from diprotic acids, which can donate two protons or hydrogen ions per molecule, and polyprotic acids, which can donate more than two.

Characteristics

Monoprotic acids are characterized by their ability to donate a single proton or hydrogen ion in a reaction. This characteristic is determined by the acid's chemical structure. The most common examples of monoprotic acids include hydrochloric acid (HCl), nitric acid (HNO3), and acetic acid (CH3COOH).

Acid Dissociation Constant

The strength of a monoprotic acid is determined by its acid dissociation constant (Ka), which measures the ratio of the concentration of the dissociated form of the acid to the undissociated form in a solution. The larger the Ka, the stronger the acid.

pH and Monoprotic Acids

The pH of a solution containing a monoprotic acid can be calculated using the Henderson-Hasselbalch equation, which relates the pH (or pOH) of a solution to the pKa (the negative log of the Ka) and the ratio of the concentrations of the dissociated and undissociated forms of the acid.

Applications

Monoprotic acids are widely used in various fields, including chemistry, biology, and medicine. They are essential in the production of many chemicals and are also used in the food industry for their preservative and flavor-enhancing properties.

See Also

• Acid
• Base
• pH
• Acid dissociation constant
• Henderson-Hasselbalch equation