Answer
The (c) statement is true.
Work Step by Step
- If the solution had a 0.1M strong acid, the pH would be = 1.
$-log[0.1] = 1$
But, since the solution is made of a weak acid, the pH will be higher than 1.
Therefore: (a) = False and (d) = False
- For a pure acid solution, if we ignore the $10^{-14}M$ of $H^+$ from water (which is negligible), the sentence ($[H^+] = [A^-]$) will be always true.
Therefore: (b) = False and (c) = True.
