Chapter 16/17 Unit Test Objectives
o Understand the three definitions of acids and bases and be able to identify
reaction species as Arrhenius acids or bases, Brønsted-Lowery acids and bases
or Lewis acids or bases
o Identify compounds as strong or weak acids or bases as well as the conjugates
of each. Understand why some acids or bases are strong and other are not.
o Convert between [H+], [OH-] and pH and pOH.
o Understand the information presented in the pH scale.
o Use ICE charts to determine the pH of various weak acids or bases and be able
to determine when a Ka is appropriate and when a Kb is appropriate for these
calculations.
o Convert between Ka and Kb using Kw.
o Apply Le Châtelier’s principle to weak acid-base equilibrium when a common ion
is present.
o Understand what a buffer is, how to identify when a buffer is present and how to
calculate the pH of a buffer using both an ICE chart and the HendersonHasselbach equation.
o Conceptually understand titration curves, the various “landmarks” that can be
found on the curves, what they mean and how these curves differ bases on the
identity of the titrant and the solution being titrated. (Recall, the “crib notes”
handed out in class and the quiz)
o Be able to perform calculations of strong acid-strong base titrations (see pg. 671673 for information and a worked out example. You may also want to try the
practice exercise on page 673 immediately following the example for extra
practice since the answers are given for you to check your work.)
o Be able to calculate the pH, pOH, [H+] and [OH-] at any point in a titration. Pay
particular attention to how to do this at the equilivance point…it gets a bit tricky
since the major species present in the solution changes here. (Recall, we
worked out a very challenging titration in class for your review. You should also
review pg. 673-677 for information, more example problems and graphic “plans
of attack.” It is also highly suggested that you try the practice exercise on pg.
676 immediately following the example and check your answers.)
o Understand and apply principles of equilibrium as it applies to solubility and
identify factors that affect solubility.
o Know what a complex ion is, their amphoteric nature and how to determine its
stability in aqueous solution using the equilibrium constant. (Note, we will not be
covering complex ion formation in depth. If you are looking to maximize your AP
test score, you may want to review Ch 24 of your text and the rules laid out in the
predicting products hand-out.)