Conjugate base
In chemistry, the term “conjugate base” refers to the species that is formed when an acid loses a proton (H+ ion)
In chemistry, the term “conjugate base” refers to the species that is formed when an acid loses a proton (H+ ion). It is the product that remains after the acid has donated its proton.
To better understand this concept, it is crucial to first grasp the concept of acids and bases. In general terms, an acid is a substance that can donate a proton (H+ ion), and a base is a substance that can accept a proton. When an acid donates a proton, it transforms into its conjugate base.
Here’s an example to illustrate this concept: Let’s consider the acid acetic acid (CH3COOH), which can donate a proton to form its conjugate base, acetate ion (CH3COO-).
CH3COOH (acetic acid) ⇌ CH3COO- (acetate ion) + H+ (proton)
In this reaction, acetic acid is the acid, and it donates a proton (H+) to form its conjugate base, acetate ion. The acetate ion now has an extra negative charge due to the gain of the proton, and it is referred to as the conjugate base of acetic acid.
It’s important to remember that the conjugate base always contains one less hydrogen atom than the acid from which it is derived. In other words, the conjugate base is formed when the acid loses a hydrogen atom along with its lone electron pair.
In summary, the conjugate base of an acid is the species that remains after the acid donates a proton. It is formed by the removal of a hydrogen atom from the acid molecule, creating a species with a negative charge. Understanding conjugate bases helps in studying acid-base reactions and the principles of equilibrium in chemistry.
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