Acid dissociation refers to the process by which an acid releases a proton (H+) into solution, forming its conjugate base and contributing to the acidity of the solution. The strength of an acid is determined by its dissociation constant (Ka), with stronger acids having higher Ka values, indicating a greater tendency to donate protons.

Acid Dissociation

Acid dissociation

acid releases a proton

A conjugate base is formed when an acid donates a proton during a chemical reaction, resulting in the acid's corresponding base. Understanding conjugate bases is essential for predicting the direction of acid-base reactions and the strength of acids and bases in solution.

conjugate base

acidity of the solution

strength of an acid

The dissociation constant (K_d) is a specific type of equilibrium constant that measures the propensity of a larger complex to dissociate reversibly into smaller components, reflecting the affinity between the components. A lower K_d value indicates a higher affinity between the components, meaning they are more likely to remain bound together under equilibrium conditions.

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