Answer
The statements (b) and (c) are true.
Work Step by Step
- For a pure acid solution, if the value of the $H^+$ from water is negligible, which it is (1.0M compared to $10^{-14}$M), the concentrations of $[H^+] and [A^-]$ will be equal.
Therefore: (a) = False
- The solution is made out of a strong acid, so:
$[H^+] = [HA]_{initial} = 1.0M$
$pH = -log[1.0M] = 0$
So: (b) = True
- In a strong acid solution, all the $[HA]$ will ionize into $[H^+]$ and $[A^-]$. Since there was 1.0M of the acid, there will be 1.0M of $[H^+]$.
So: (c) = True.
- After the ionization of a strong acid, the acid's concentration is zero, because it all got ionizated.
So: (d) = False
