Weak vs. strong acid dissociation determines pH Steps:

• Classify solutions: CH3COOH (Acid 1) is weak acid; HCl (Acid 2) is strong acid.
• Strong acids fully dissociate at 0.1 M, yielding [H+] = 0.1 M (pH = 1).
• Weak acids partially dissociate; pH = 4 for Acid 1 means [H+] = 10^{-4} M, much lower than 0.1 M.
• Lower dissociation in weak acids explains higher pH compared to strong acids.

Why C is correct:

• Weak acids dissociate less completely than strong acids, per the definition of acid strength and Ka values (e.g., Ka for CH3COOH ≈ 10^{-5}).

Why the others are wrong:

• A: pH of Acid 2 not given; not enough information to compare pH values or attribute to solubility (both acids are soluble).
• B: pH 11 (Base 1) gives [OH-] = 10^{-3} M; pH 14 (Base 2) gives higher [OH-]; Base 1 has lower [OH-].
• D: pH 14 for 0.1 M Base 2 implies [OH-] = 1 M, inconsistent with 0.1 M concentration; not enough information.

Final answer: C