The correct statement among the options provided is:
The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.
This is true because hydrochloric acid (HCl) is a strong acid and fully dissociates in solution, resulting in a very large dissociation constant (Ka). In contrast, acetic acid (CH₃COOH) is a weak acid and does not fully dissociate, leading to a much smaller dissociation constant.
Here’s a breakdown of the other options:
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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 might not necessarily be true because it depends on the initial concentrations of the acids. HCl fully dissociates, while acetic acid does not.
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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 is generally true for equal concentrations, as HCl being a strong acid produces more H₃O⁺ ions than acetic acid. However, it must be noted that the exact pH values vary based on their respective concentrations.
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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 false. A strong acid like HCl will produce more H₃O⁺ ions than a weak acid like acetic acid, assuming equal initial concentrations.
In conclusion, the most accurate and unambiguous statement is about the dissociation constants.
1 answer