Chemistry (7th Edition)

Published by Pearson
ISBN 10: 0321943171
ISBN 13: 978-0-32194-317-0

Chapter 16 - Applications of Aqueous Equilibria - Section Problems - Page 709: 50


(a) $pH = 7.00$ (b) $pH > 7.00$ (c) $pH < 7.00$ (d) $pH > 7.00$

Work Step by Step

1. Identify which compound is stronger; the solution will have its characteristics: (b) $Ba(OH)_2$ Strong base, $HOI$ Weak acid. The base is the stronger one: Basic solution, $pH > 7$ (c) $HBr$ Strong acid, $C_6H_5NH_2$ Weak base. The acid is the stronger one: Acidic solution, $pH < 7$ (d) $HNO_2$ Weak acid, $KOH$ Strong base. The base is the stronger one: Basic solution, $pH > 7$ 2. When we have 2 strong compounds, the solution will be neutral, because they are going to completely neutralize each other. (a) $HNO_3$ Strong acid, $KOH$ Strong base. Both have the same strength: Neutral solution, $pH = 7$ Why does that happen? When we mix, for example: $Ba(OH)_2$ and $HOI$, this is the reaction: $Ba(OH)_2(aq) + HOI(aq) -- \gt Ba^{2+}(aq) + OI^-(aq) + H_2O(l)$ Now, let's analyze each product: $Ba^{2+}$: No significant acidity/basicity; $OI^-$: Weak base; Since we only have a base acting in the solution, it will be a basic one. When we have a strong acid and a strong base: $HNO_3(aq) + KOH(aq) -- \gt H_2O(l) + K^+(aq) + NO{_3}^-(aq)$ $K^+$: No significant acidity/basicity; $N{O_3}^-$: No significant acidity/basicity; Therefore, the solution will be neutral.
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