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
- The strength of an acid is determined by its ability to ionize in water; strong acids ionize completely, while weak acids do not.
- Acid ionization can be represented by a chemical equation, such as $HA \rightleftharpoons H^+ + A^-$ for a generic acid $HA$.
- $K_a$ values are used to compare the strengths of different acids; larger $K_a$ values indicate stronger acids.
- The degree of ionization affects the pH of the solution; higher degrees lead to lower pH values.
- In dilute solutions, the percentage of ionization increases because there are fewer acid molecules competing for dissociation.
Review Questions
- What does the $K_a$ value tell you about an acid's strength?
- How is acid ionization represented in a chemical equation?
- What happens to the pH of a solution as the degree of ionization of an acid increases?
"Acid ionization" appears in:
Study guides (1)
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.
