Acid ionization

Definition

Acid ionization is the process by which an acid releases protons ($H^+$) into solution, forming its conjugate base. This process is quantified by the acid dissociation constant, $K_a$.

5 Must Know Facts For Your Next Test

1. The strength of an acid is determined by its ability to ionize in water; strong acids ionize completely, while weak acids do not.
2. Acid ionization can be represented by a chemical equation, such as $HA \rightleftharpoons H^+ + A^-$ for a generic acid $HA$.
3. $K_a$ values are used to compare the strengths of different acids; larger $K_a$ values indicate stronger acids.
4. The degree of ionization affects the pH of the solution; higher degrees lead to lower pH values.
5. In dilute solutions, the percentage of ionization increases because there are fewer acid molecules competing for dissociation.

Related terms

Conjugate Base:

The species that remains after an acid has donated a proton ($H^+$).

$pK_a$: The negative logarithm of the acid dissociation constant ($K_a$), used to express acidity.

$H^+$ (Proton): A hydrogen atom that has lost its electron, commonly referred to as a proton in acid-base chemistry.