Additional Aspects of   Equilibria

	17.1	Predict qualitatively and calculate quantitatively the effect of an added common ion on the pH of an aqueous solution of a weak acid or base.
	17.2	Describe how a buffer solution of a particular pH is made and how it operates to control pH.
	17.3	Calculate the change in pH of a simple buffer solution of known concentration caused by adding a small amount of strong acid or base.
	17.4	Calculate the concentrations of each species present in a solution formed by mixing an acid and a base.
	17.5	Describe the form of the titration curves for a strong acid by a strong base, a weak acid by a strong base, or a strong acid by a weak base.
	17.6	Calculate the pH at any point, including the equivalence point, in acid-base titrations.
	17.7	Set up the expression for the solubility-product constant of a salt.
	17.8	Calculate Ksp from solubility data and solubility from the value of Ksp.
	17.9	Calculate the effect of an added common ion on the solubility of a slightly soluble salt.
	17.10	Explain the effect of pH on a solubility equilibrium involving a basic or acidic ion.
	17.11	Formulate the equilibrium between a metal ion and a Lewis base to form a complex ion of a metal.
	17.12	Describe how complex formation can affect the solubility of a slightly soluble salt.
	17.13	Calculate the concentration of a metal ion in equilibrium with a ligand with which it forms a soluble complex ion, from a knowledge of initial concentrations of Kf.
	17.14	Explain the origin of amphoteric behavior and write equations describing the dissolution of an amphoteric metal hydroxide in either an acidic or basic medium.
	17.15	Predict whether a precipitate will form when two solutions are mixed, given appropriate Ksp values.
	17.16	Explain the general principles that apply to the groupings of metal ions in the qualitative analysis of an aqueous mixture.

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