Which of the following statements is true about acids and their strength based on Ka values?

The assertion that larger Ka values indicate stronger acids is fundamental to understanding acid strength in chemistry. The acid dissociation constant, Ka, measures the extent to which an acid dissociates in water to form hydronium ions (H₃O⁺) and its corresponding conjugate base. A higher Ka value signifies that the acid dissociates more completely in solution, resulting in a greater concentration of hydronium ions, which characterizes a stronger acid.

In essence, when an acid has a large Ka, it means that the equilibrium position of the dissociation reaction lies significantly toward the products, meaning more of the acid is present in the form of ions in solution compared to the undissociated form. Consequently, stronger acids are characterized by larger Ka values.

As a point of context, weaker acids, represented by lower Ka values, imply that the dissociation is less favorable, resulting in fewer hydronium ions compared to their undissociated form. This relationship is further illustrated by the concept of pKa, where weaker acids have higher pKa values, reflecting lower Ka values. Thus, the larger the Ka, the stronger the acid, reinforcing the truth of the correct statement regarding acid strength.