Final answer:
The percent dissociation of a weak acid in solution depends on both the acid dissociation constant (Ka) and the initial concentration of the acid (C), hence the answer to the question is true.
Step-by-step explanation:
The percent dissociation of a weak acid in solution depends both on the acid ionization constant (Ka) and the initial concentration of the acid (C). The percent dissociation indicates how much of the acid dissociates into its ions in solution. For a weak acid, when the concentration of the weak acid is high, the percent dissociation is lower because the solution can reach equilibrium with a smaller fraction of dissociated ions. On the other hand, if you have a lower concentration of the acid, the percent dissociation increases as more of the acid must dissociate to reach equilibrium. The Ka reflects the strength of the acid; stronger acids have larger Ka values and dissociate more in water, which in turn affects the percent dissociation.
The quadratic equation derived from the acid dissociation equilibrium is used to solve for the concentration of hydronium ions (H3O+) in solution. For a weak acid dissociating in water, the equilibrium constant is referred to as Ka, and the dissociation can be considered by the reaction HA (aq) + H2O → H3O+ (aq) + A- (aq) with the corresponding expression for the acid dissociation constant: Ka = [H3O+][A-] / [HA].
Therefore, the correct answer to the question posed is true; percent dissociation does indeed depend on both the acid dissociation constant (Ka) and the initial concentration of the acid (C). hence the answer to the question is true.