The following objectives should be achieved by the student during this course. All of the objectives are preceded by the phrase, "The student should be able to:"

l. List the qualities of
a primary standard.

2. Distinguish between
a primary standard and a secondary standard.

3. Define the grades of
chemicals (ACS, primary standard tech., etc.).
**4. $Treat analytical
data statistically and be able to determine if a questionable result should
be rejected.**

5. Describe substitution
weighing and give the advantages of substitution weighing. (This would
include defining any terms listed as an advantage.)

6. Describe how to obtain
a suitable analytical sample and give the properties of suitable analytical
samples.

7. Apply chemical equilibrium
data to perform quantitative analysis.
**8. $Work the assigned
problems.**

9. Apply chemical equilibrium
principles to determine the equilibrium expressions for dissociations and
formations; also, work any associated problems.

10. Define acids and bases.

11. Apply the Bronsted
Definition to given cases--especially the idea of conjugate acids and bases;
also, apply to buffers.

12. Given the pH, calculate
the H^{+} molarity; or, given the H^{+} molarity, calculate
the pH (pOH).

13. Calculate the pH of
the following types of aqueous solutions: (In each case, ionization constants
and concentrations will be given.) weak acids, weak bases, buffers, salts
of strong acids and strong bases, salts of strong acids and weak bases,
salts of strong bases and weak acids, salts of weak acids and weak bases,
strong acids, strong bases.

14. Recognize and apply
multiple equilibria situations.

15. Define titration and
list the requirements for a titration.

16. Calculate titration
problems (including back titrations).

17. Define buffer capacity
and work associated problems.

18. Explain acid-base
indicators, and show why the change is over a 2 pH unit change.

19. Construct a titration
curve for a weak acid-strong base titration or for a weak base-strong acid
titration.

20. Given a titration
curve for a weak acid-strong base (or weak base-strong acid), identify
the regions, give the pKa or pKb for the substance titrated, discuss the
feasibility of the titration, calculate either percent pure or equivalent
weight.

21. Discuss the application
of acid-base titrations--include Kjdahl, carbonate, and other applications.

22. List the types of
literature sources in the chemical literature. Also, define and give illustrations
of each type of literature.

23. Give one example of
each type of literature source in 22 that applies to analytical chemistry.

24. List the steps that
you would take in searching for a suitable analytical method for the analysis
of your real life determination.

25. Define gravimetric
analysis.

26. List the requirements
for a suitable gravimetric determination.

27. Discuss factors which
limit the purity of precipitates, and describe how to insure pure precipitates.

28. Define homogeneous
precipitation, give the advantages of the method, and give an example of
the method.

29. Define and state the
applications and advantages of the following: carriers in trace analysis,
colloids, peptization, gravimetric factors, masking agents, inhibitors,
digestion, filtration, ignition, constant weight, post precipitation, co-precipitation,
and washing of precipitates. List an example of each of the items listed,
and point out both pitfalls and disadvantages of each of the items listed.

30. List the requirements
for precipitation titration methods and for complexometric titration methods.

31. Demonstrate an understanding
of gravimetric factors by use in gravimetric determinations and in working
related problems.

32. List and describe
the methods used for determining the endpoint in precipitation titration
methods. Note any conditions required for a given method (i.e., pH control,
etc.).

33. Compare and contrast
monodentate ligands and chelates for suitable complexometric titrants.

34. List and explain the
uses of complexes in analysis, also give examples of each use.

35. Describe the effect
of pH and pK formation on complexometric titrations.

36. Describe the effect
of pH on redox titration methods.

37. Given a titration
curve (pH, ppt., complexometric, or redox), and determine the feasibility
of the titration method.

38. List the types of
EDTA (or complexometric) titration methods. Give an example of each type.

39. Be able to determine
both Ca and Mg concentrations in hard water.

40. List the criteria
for selection of an indicator for complexometric titration methods.

41. Define the following
types of solvents: amphiprotic, non-ionizable, aprotic (inert). Give an
example of the use of each of the types in both titrations and in solvent
extraction.

42. Define Ion Exchange
methods, and list the criteria and limitations.

43. Apply Ksp values to
see what will precipitate first and what concentrations will be left in
solution.

44. Discuss the advantages
and disadvantages of the methods of aliquots.

45. Define oxidation,
reduction, oxidizing agent, reducing agent, and apply to given equations.

46. List and discuss the
requirements for redox volumetric determinations.

47. Calculate the direction
of a reaction and Keq from E^{o} values.

48. Determine if a redox
reaction is quantitative from E^{o} values.

49. Discuss the types
of redox titration indicators.

50. Discuss the use, preparation,
advantages and disadvantages of:

K_{2}Cr_{2}O_{7}, KMnO_{4}, Ce(SO_{4})_{2},
and I_{2} as oxidizing agents;

and As_{2}O_{3}, FeSO_{4} (NH_{4})_{2}SO_{4},
Na_{2}S_{2}O_{3}, and iron wire as reducing agents.

51. Apply the Nernst equation
to given situations.

52. List and discuss problems
associated with real-life samples.

53. List and discuss problems
associated with the location and selection of a method of determination.

54. *List and discuss
the requirements for an electrogravimetric (electrodeposition) determination.

55. *List and discuss
the requirements for a controlled current coulometric titration.

56. *Define and discuss
the following: overvoltage, deposition potential, current efficiency, 96,500.

57. *List and discuss
the desired properties of a good electroplate. Include those factors which
are needed to produce a good plate.

58. Define Beer's Law
and relate it to %T. (A = abc; A = e
bc; -log_{10}T = A)

59. List the requirements
for a quantitative spectrophotometric determination.

60. List and discuss the
requirements for liquid-liquid extraction.

61. Discuss the number
of extractions and the volume of extractant per extraction.

62. Discuss the importance
and types of separations in Analytical Chemistry.

63. Discuss percent extracted
(%E) and factors relating to percent extracted.
**64.$ Treat all data
using Excel and appropriate statistical tests.**

_________

* May not be covered.
Check with Dr. Sherren.

$ Objective that applies
all term.

2/26/01