Chemistry (7th Edition)

Published by Pearson

Chapter 16 - Applications of Aqueous Equilibria - Worked Example - Page 664: 5

Answer

- The second solution (2) has the highest pH; - The first solution has the greater $HF$ dissociation;

Work Step by Step

- The presence of $F^-$ ions in the second solution makes its pH greater than the pure $HF$ one, because the fluoride ion can act as a base. - Due to the common ion effect, the presence of $F^-$ in the second solution restricts the dissociation of $HF$, because it moves the equilibrium to the left side: $HF(aq) + H_2O(l) \lt -- \gt F^-(aq) + H_3O^+(aq)$ Therefore, the first solution has the greater $HF$ percent dissociation.

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