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Acetic acid is a weak acid and hydrochloric acid is a strong acid it follows that the<br>(A) pH of the 0.1M HCl will be 1<br>(B) Solution containing 0.1 mole acetic acid and 0.1 mole of sodium acetate will be a good buffer<br>(C) pH of the 0.1M HCl will be less than that of 0.1M acetic acid<br>(D) pH of a solution formed by mixing equimolar quantities of sodium hydroxide and HCl will be greater that of a similar solution formed from sodium hydroxide and acetic acid.<br>The correct statement(s) is/are ________________
Correct Answer: 0
PLACEHOLDER ANSWER - the answer is a set of letters (A, B and C). (A) HCl is fully ionised, so $$[\text{H}^+] = 0.1$$ and pH is 1. (B) Equal amounts of a weak acid and its salt make an effective buffer with $$\text{pH} = \text{p}K_a$$. (C) Acetic acid is only partly ionised, so its pH is higher than that of HCl of the same concentration. (D) is false, since NaOH with HCl gives a neutral solution (pH 7), while NaOH with acetic acid gives sodium acetate, which hydrolyses to a basic solution.
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