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:
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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.
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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.
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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.
1 answer