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Learning Objectives
By the end of this section, you will be able to:
Write chemical equations and equilibrium expressions representing solubility equilibria
Carry out equilibrium computations involving solubility, equilibrium expressions, and solute concentrations
Solubility equilibria are established when the dissolution and precipitation of a solute species occur at equal rates. These equilibria underlie many natural and technological processes, ranging from tooth decay to water purification. An understanding of the factors affecting compound solubility is, therefore, essential to the effective management of these processes. This section applies previously introduced equilibrium concepts and tools to systems involving dissolution and precipitation.
The Solubility Product
Recall from the chapter on solutions that the solubility of a substance can vary from essentially zero (insoluble or sparingly soluble) to infinity (miscible). A solute with finite solubility can yield a saturated solution when it is added to a solvent in an amount exceeding its solubility, resulting in a heterogeneous mixture of the saturated solution and the excess, undissolved solute. For example, a saturated solution of silver chloride is one in which the equilibrium shown below has been established.
AgCl(s)⇌precipitationdissolutionAg+(aq)+Cl−(aq)
In this solution, an excess of solid AgCl dissolves and dissociates to produce aqueous Ag+ and Cl– ions at the same rate that these aqueous ions combine and precipitate to form solid AgCl (Figure 15.2). Because silver chloride is a sparingly soluble salt, the equilibrium concentration of its dissolved ions in the solution is relatively low.
Figure 15.2 Silver chloride is a sparingly soluble ionic solid. When it is added to water, it dissolves slightly and produces a mixture consisting of a very dilute solution of Ag+ and Cl– ions in equilibrium with undissolved silver chloride.
The equilibrium constant for solubility equilibria such as this one is called the solubility product constant, Ksp, in this case
AgCl(s)⇌Ag+(aq)+Cl−(aq)Ksp=[Ag+(aq)][Cl−(aq)]
Recall that only gases and solutes are represented in equilibrium constant expressions, so the Ksp does not include a term for the undissolved AgCl. A listing of solubility product constants for several sparingly soluble compounds is provided in Appendix J.
EXAMPLE 15.1
Writing Equations and Solubility Products
Write the dissolution equation and the solubility product expression for each of the following slightly soluble ionic compounds:
(a) AgI, silver iodide, a solid with antiseptic properties
(b) CaCO3, calcium carbonate, the active ingredient in many over-the-counter chewable antacids
(c) Mg(OH)2, magnesium hydroxide, the active ingredient in Milk of Magnesia
(d) Mg(NH4)PO4, magnesium ammonium phosphate, an essentially insoluble substance used in tests for magnesium
(e) Ca5(PO4)3OH, the mineral apatite, a source of phosphate for fertilizers
Solution
(a)AgI(s)⇌Ag+(aq)+I−(aq)Ksp=[Ag+][I−](b)CaCO3(s)⇌Ca2+(aq)+CO32−(aq)Ksp=[Ca2+][CO32−](c)Mg(OH)2(s)⇌Mg2+(aq)+2OH−(aq)Ksp=[Mg2+][OH−]2(d)Mg(NH4)PO4(s)⇌Mg2+(aq)+NH4+(aq)+PO43−(aq)Ksp=[Mg2+][NH4+][PO43−](e)Ca5(PO4)3OH(s)⇌5Ca2+(aq)+3PO43−(aq)+OH−(aq)Ksp=[Ca2+]5[PO43−]3[OH−]
Check Your Learning
Write the dissolution equation and the solubility product for each of the following slightly soluble compounds:
(a) BaSO4
(b) Ag2SO4
(c) Al(OH)3
(d) Pb(OH)Cl
ANSWER:
(a)BaSO4(s)⇌Ba2+(aq)+SO42−(aq)Ksp=[Ba2+][SO42−];(b)Ag2SO4(s)⇌2Ag+(aq)+SO42−(aq)Ksp=[Ag+]2[SO42−];(c)Al(OH)3(s)⇌Al3+(aq)+3OH−(aq)Ksp=[Al3+][OH−]3;(d)Pb(OH)Cl(s)⇌Pb2+(aq)+OH−(aq)+Cl−(aq)Ksp=[Pb2+][OH−][Cl−]
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