CHEM 122 11th Edition Lecture 30Outline of Last LectureI. Buffer Solutionsa. Ideal Bufferb. Henderson-Hasselbalch EquationII. Change in pH of a Buffer SolutionIII. Acid-Base TitrationsIV. Solubility Equilibriuma. Solubility Product ConstantV. Ion ProductsOutline of Current Lecture I. Factors that affect solubilityII. Precipitations of IonsCurrent LectureFactors that affect solubility:- Although Ksp is indeed constant, the position of equilibrium can be affected by the adding common ions.- Common ions: an ion that is common between to substances Ex. AgCl and NaCl. Cl would be the common ion.- Addition of a substance to a saturated solution creates the ion product to exceed the Kspvalue. The ion concentration must be reduced until the ion product equals the Ksp value.- The equilibrium will then shift to the left to make up for it, but the value of Ksp is unchanged.Precipitation of ions:These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best Used as a supplement to your own notes, not as a substitute.- Ion scan be predicated from a solution when the ion product exceeds the solubility product constant.- This can be achieved by adding a common ion or an ion that has a smaller Ksp.- Q>Ksp, precipitation occurs until Q=K- Q=Ksp, at equilibrium, a saturated solution has formed.- Q<Ksp, more solid needs to dissolve until
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