Question

Which of these statements is/are true regarding a 1.0 M solution of a strong acid HA? (a) [A−] > [H+] true false (b) The pH is 0.0. true false (c) [H+] = 1.0 M true false (d) [HA] = 1.0 M true false

Answer 1

Answer:

(a) false, (b) true, (c) true and (d) false

Explanation:

HA is a strong acid. Hence it dissociates completely to produce equal amount of $H^{+}$ and $A^{-}$ as follows:

                                  $HA\rightarrow H^{+}+A^{-}$

Hence no HA will be left in solution.

$pH=-log[H^{+}]$ , where $[H^{+}]$ represents concentration of $H^{+}$ in molarity

Here, $[H^{+}]=1.0M$

So, $pH=-log(1.0)=0$

Hence, (a) false, (b) true, (c) true and (d) false