Chapter 17 - Learning Goals

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.

Calculate the concentration of each species present in a solution formed by mixing an acid and a base.

Describe the form of the titration curve for the titration of a strong acid by a strong base; a strong base by a strong acid; a weak acid by a strong base; and a weak base by a strong acid.

Calculate the initial pH; the pH at the equivalence point, and the pH at ½ way to the equivalence point for titrations involving weak acid/strong base or weak base/strong acid titrations.

Describe how a buffer solution of a particular pH is made, and the reactions that allow it to control pH.

Calculate the change in pH of a simple buffer solution of known composition caused by adding a small amount of strong acid or base.

Set up the expression for the solubility-product constant for a salt.

Calculate Ksp from solubility data, and solubility from the value of Ksp.

Calculate the effect of an added common ion on the solubility of a slightly soluble salt.

Predict whether a precipitate will form when two solutions are mixed, given appropriate Ksp values.

Explain the effect of pH on a solubility equilibrium involving a basic or acidic ion.

Formulate the equilibrium between a metal ion and a Lewis base to form a complex ion of a metal.

Describe how complex formation can affect the solubility of a slightly soluble salt.

Calculate the concentration of a metal ion in equilibrium with a Lewis base with which it forms a soluble complex ion, from a knowledge of initial concentrations and Kf.