Which of these statements about how the percent ionization of a weak acid depends on acid concentration is true? (a) Line A is most accurate because Ka does not depend on concentration. (b) Line A is the most accurate because the percent ionization of the acid does not depend on concentration (c) Line B is the most accurate because as the acid concentration increases, a greater proportion of it is ionized. (d) Line B is the most accurate because as the acid concentration increases, Ka increases. (e) Line C is the most accurate because as the acid concentration increases, a lesser proportion of it ionized. (f) Line C is the most accurate because as the acid concentration increases, Ka decreases.

Answer: E

Line C is the most accurate because as the acid concentration increases, a lesser proportion of it ionized.

e.) Line C is the most accurate because as the acid concentration increases, a lesser proportion of it ionized.

Explanation:

The strengths of acids can be described as by the extent to which it ionize in aqueous solution. Acid can react with alot of solutions such as water.

In addition, with the measurements of equilibrium constants in aqueous solutions, We can determine the relative strengths of acids. Strong acid ionize to some extent while in a solutions of the same concentration, to yield higher concentrations of hydronium ions much more than the weak acids. The equilibrium constant for an acid is reffered to as "acid-ionization constant" (Ka). The reaction of the acid is described below;

HA

(aq) + H2O (l) ⇌H3O + (aq) + A - (aq)

Therefore, Line C is the most accurate because as the acid concentration increases, a lesser proportion of it ionized