## Chemistry 12th Edition

- 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