(e) Ca 5(PO 4) 3OH, the mineral apatite, a source of phosphate for fertilizers (d) Mg(NH 4)PO 4, magnesium ammonium phosphate, an essentially insoluble substance used in tests for magnesium (c) Mg(OH) 2, magnesium hydroxide, the active ingredient in Milk of Magnesia (b) CaCO 3, calcium carbonate, the active ingredient in many over-the-counter chewable antacids
(a) AgI, silver iodide, a solid with antiseptic properties Write the dissolution equation and the solubility product expression for each of the following slightly soluble ionic compounds: Writing Equations and Solubility Products For example, a saturated solution of silver chloride is one in which the equilibrium shown below has been established. 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. Recall from the chapter on solutions that the solubility of a substance can vary from essentially zero ( insoluble or sparingly soluble) to infinity ( miscible). This section applies previously introduced equilibrium concepts and tools to systems involving dissolution and precipitation. An understanding of the factors affecting compound solubility is, therefore, essential to the effective management of these processes. These equilibria underlie many natural and technological processes, ranging from tooth decay to water purification.
Solubility equilibria are established when the dissolution and precipitation of a solute species occur at equal rates. Carry out equilibrium computations involving solubility, equilibrium expressions, and solute concentrations.Write chemical equations and equilibrium expressions representing solubility equilibria.By the end of this section, you will be able to:
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