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.

Review Questions

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.