The correct statement about hydrochloric acid (HCl) and acetic acid (CH₃COOH) is:
The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.
Here's the reasoning for each statement:
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The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.
This statement is correct because HCl is a strong acid that fully dissociates in solution, while acetic acid is a weak acid that only partially dissociates. Therefore, the dissociation constant (Ka) for acetic acid is significantly less than that of hydrochloric acid. -
The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid.
This statement is usually correct for solutions of equivalent concentrations; hence this statement can be true in many cases but not universally true without specifying concentrations. -
If the initial concentration of each acid is the same, then acetic acid will produce more H₃O⁺ ions than hydrochloric acid.
This statement is false because HCl, being a strong acid, will fully dissociate and produce more H₃O⁺ ions than acetic acid at the same concentration. -
A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium.
This statement is not necessarily true because the total concentrations can vary based on the initial concentrations of the acids involved.
Thus, the only emphatically correct statement about HCl and acetic acid is regarding their dissociation constants.