Chapter 15 - Acid-Base Equilibria

endpoint

The ________ is defined by the change in color of the indicator.

indicator

Choosing a(n) ________ is easier if there is a large change in pH near the equivalence point of the titration.

Ksp

________ is an equilibrium constant; solubility is an equilibrium position.

equivalence point

The ________ is defined by the reaction stoichiometry.

anion

If the ________ of the solid is a good base, the solubility is greatly increased by acidifying the solution.

solubility product

The ________ is an equilibrium constant and has only one value for a given solid at a given temperature.

Pure liquids

________ and pure solids are never included in an equilibrium expression.

stable complex ions

In cases where the anion is not sufficiently basic, the ionic solid often can be dissolved in a solution containing a ligand that forms ________ with its cation.

Metal ions

________ and ligands one at a time in steps characterized by equilibrium constants called formation constants for stability constants.

common ion effect

The ________ is an application of Le Châteliers principle.

Indicators

________ are sometimes used to mark the equivalence point of an acid- base titration.

equivalence point

For a strong base- weak acid titration, the pH is greater than 7 at the ________ because of the basic properties.

common ion effect

The ________ is an application of Le Châtelier’s principle

buffered solution

A ________ is one that resists a change in its pH when either hydroxide ions or protons are added.