Chemistry 12th Edition

- 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.