Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?(1 point)

The correct statement among the options provided is:

**The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.**

Hydrochloric acid (HCl) is a strong acid that completely dissociates in water, leading to a very high dissociation constant (Ka) that can be considered as being effectively infinite for practical purposes. Acetic acid (CH3COOH), on the other hand, is a weak acid that only partially dissociates in solution, resulting in a much smaller Ka value. Therefore, the dissociation constant for HCl is indeed greater than that for acetic acid.

The other options are incorrect for the following reasons:

1. **A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium.** - This is not necessarily true, as the actual concentration of solute depends on the starting concentrations and does not inherently mean HCl in solution is more concentrated than a comparable acetic acid solution.

2. **The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid.** - This statement is generally true as HCl being a strong acid would lead to a lower pH compared to acetic acid at the same initial concentration. However, if the concentrations were different, it might not hold.

3. **If the initial concentration of each acid is the same, then acetic acid will produce more H3O+ ions than hydrochloric acid.** - This is incorrect because HCl will produce more H3O+ ions upon dissociation compared to acetic acid at the same initial concentration.

Thus, the most accurate and definitively correct statement is about the dissociation constants.