Describe the effect of common ions on the ionization of weak acids
and bases, and calculate the concentrations of all species present in solutions
of weak acids or bases and their common ions.
Explain why the pH of water changes markedly when a small amount of
H3O+ or OH- is added, and why the pH of a buffer does not
change very much with a similar addition.
Describe how buffer solutions can be prepared.
Know the limitations of the basic equations used to determine the pH of
buffer solutions (specifically the Henderson-Hasselbalch equation) by
understanding their derivations.
Calculate the pH of a buffer solution from concentrations of the buffer
components and a value of Ka or Kb, and describe how to prepare a
buffer that has a specific pH.
Determine the changes in pH of buffer solutions that result from the
addition of acids or bases.
Define and compute values for: "buffer range" and "buffer capacity."
Explain how an acid-base indicator works to determine the equivalence point
in a titration.
Calculate pH values and plot the titration curve of a strong acid with a
strong base, or a strong base with a strong acid.
Calculate pH values and plot the titration curve of a weak acid with a
strong base or of a weak base with a strong acid.
Plot titration curves and use those curves to determine the initial pH,
buffer region, and the pH of the equivalence point, and to select an
appropriate indicator.