AUTOPROTOLYSIS Meaning and
Definition
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Autoprotolysis is a chemical process in which a substance, typically a solvent or a compound capable of acting as an acid or a base, donates or accepts a proton from itself, resulting in the formation of both a conjugate acid and a conjugate base. This self-ionization phenomenon occurs in pure substances in the absence of an external source of a protons or hydroxide ions.
In the case of water, autoprotolysis is commonly referred to as self-ionization. Two water molecules can transfer a proton between them, forming a hydroxide ion (-OH) and a hydronium ion (H3O+). The chemical equation representing this process is H2O + H2O ⇌ H3O+ + OH-, where the double arrow indicates that the reaction can proceed in both directions.
Autoprotolysis is also observed in other solvents, such as liquid ammonia or acetic acid. These solvents can undergo self-ionization when acting as both an acid and a base. For example, acetic acid (CH3COOH) can donate a proton to another acetic acid molecule, producing an acetate ion (CH3COO-) and a hydronium ion (H3O+).
The concept of autoprotolysis is important in understanding the behavior of acids and bases in solution, as it provides insights into their self-ionization and equilibrium reactions. It is also relevant in the field of chemistry as it helps in understanding the properties and behavior of various solvents and their ability to act as acids or bases.
Etymology of AUTOPROTOLYSIS
The word "autoprotolysis" is derived from combining three Greek roots: "auto" meaning "self", "proto" meaning "first" or "primary", and "lysis" meaning "loosening" or "splitting". In chemistry, "autoprotolysis" refers to the process of self-ionization or self-dissociation of a substance in which molecules of the same substance react with each other to form ions.
