Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 17 - Additional Aspects of Aqueous Equilibria - Exercises - Page 770: 17.59a


The amount of solid $CaF_2$ in the beaker will increase.

Work Step by Step

1. This is the solubility equilibrium: $CaF_2(s) \lt -- \gt Ca^{2+}(aq) + F^-(aq)$ 2. When we add a common ion ($Ca^{2+}$ from $CaCl_2$), the equilibrium will move. According to the Le Chatelier's principle, the equilibrium will move to the $CaF_2(s)$ side. This occurs because the equilibrium will try to consume the $Ca^{2+}$, since we added more to the solution.
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