Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 15 - Additional Aqueous Equilibria - Questions for Review and Thought - Topical Questions - Page 693b: 50c


$Ca_3(PO_4)_2(s) \lt -- \gt 3Ca^{2+}(aq) + 2P{O_4}^{3-}(aq)$ $K_{sp} (Ca_3(PO_4)_2) = [Ca^{2+}]^3[P{O_4}^{3-}]^2$

Work Step by Step

- Calcium $(Ca^{2+})$ phosphate $(P{O_4}^{3-})$: $Ca_3(PO_4)_2$ 1. Write the dissociation equation for this salt: - Identify the ions of the salt: $(Ca^{2+})$ and $(P{O_4}^{3-})$, these are the products, and the reactant is the solid salt. $Ca_3(PO_4)_2(s) \lt -- \gt Ca^{2+}(aq) + P{O_4}^{3-}(aq)$ - Balance the equation: $Ca_3(PO_4)_2(s) \lt -- \gt 3Ca^{2+}(aq) + 2P{O_4}^{3-}(aq)$ 2. Now, write the $K_{sp}$ expression. - Multiply the concentrations of the ions: - The equilibrium coefficients represent the exponent of these concentrations: $K_{sp} (Ca_3(PO_4)_2) = [Ca^{2+}]^3 \times [P{O_4}^{3-}]^2$
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