CH231 - Quantitative Analysis
Fall 2004 Semester
CH231 Quantitative Chemistry I (4 semester credits)
This course is the beginning part of a two semester course in Analytical
Chemistry. This course will focus on the theory and principles of quantitative
chemical analysis and the application of these principles to solve quantitative
chemical problems.
Required:
Quantitative Chemical Analysis, 6th Edition, by Daniel C. Harris
Laboratory Notebook
Chemical Splash Goggles, indirect venting only
State Council of State Science Supervisors:
http://www.csss-science.org/safety.shtml
http://www.csss-science.org/downloads/scisafe.pdf
Optional:
Solutions Manual for Quantitative Chemical Analysis by Daniel C.
Harris
Instructor:
Dr. Barb Keller, CRW 319 (phone: 635-2438)
Office Hours:
MW
T
9:00- 11:00
10:30 – 11:30
Course Objectives: Upon completion of this course, the student should be able to:
(Chapter emphasizing each outcome is provided)
Chapters 1 & 2:
 understand and use the SI system of measurements to convert between units
 express chemical concentrations as molarity, molality, percent composition,
parts per million, and parts per billion
 describe methods for preparing chemical (electrolyte) solutions
 understand the concepts of chemical dilutions, electrolyte solutions, and
stoichiometry and be able to use these concepts to solve chemical problems
 be familiar with analytical tools that include analytical balances, burets, pipets,
volumetric glassware and analytical techniques that include filtration, drying,
and ignition.
Chapter 3:
 understand the concept of significant figures and correctly use significant
figures when performing arithmetic operations
 know what is meant by accuracy and precision and absolute and relative
uncertainty

be familiar with measurement errors, including systematic errors and random
errors
Chapter 4:
 comprehend the basic concepts from statistics that are widely used in
analytical chemistry, including Gaussian distribution, standard deviation,
mean, confidence intervals, variance,
 calculate means, standard deviations, and confidence intervals for sets of
analytical data
 understand and use the student t test to compare one different sets of
measurements with one another
 use the Q test to test for bad data
Chapter 5:
 prepare a calibration curve
 use the method of least squares to find the best straight line
 understand how the methods of standard additions and internal standards are
used in quantitative chemical analysis
 solve quantitative chemical problems relating to the concepts presented in the
chapter
Chapter 27:
 describe gravimetric analysis and combustion analysis and understand how
these concepts are used in analytical chemistry
 understand the process of precipitation
 perform gravimetric and gravimetric combustion calculations
Chapter 6:
 discuss and understand the concept of chemical equilibrium
 write the equilibrium constant expression for chemical reactions
 use Le Chatelier’s principle to predict the direction in which a chemical
system proceeds
 determine reaction quotients for chemical reactions
 understand the chapter concepts of solubility product, common ion effect, pH,
acid-base strengths and how they relate to chemical equilibria
 solve quantitative chemical equilibrium calculations
Chapter 7:
 describe and construct an acid base titration, including the determination of
the equivalence point
 perform titration calculations
Chapter 8:


understand and calculate solution ionic strengths; activities; and activity
coefficients
determine the effect that common ions and pH have one the activity of a
solution and its ionic equilibrium
Chapter 9:
 understand and use the systematic treatment of ionic equilibrium to deal with
all types of chemical equilibria
 be able to determine charge balances and mass balances for chemical
equilibria
 solve quantitative equilibrium problems using the techniques described in this
chapter.
Chapter 10:
 comprehend the distinctions between strong acids/bases and weak acids/bases
 perform typical analytical calculations for strong acids and bases
 perform typical analytical calculations for weak acids and bases
 understand the concept of conjugate acids and bases and their relative
strengths compared to the complimenting acid and base
 use equilibrium expressions to solve chemical calculations
 understand and know when to use the Henderson-Hasselbalch equation to
solve chemical calculations
 describe what a buffer is and how it is prepared
Chapter 11:
 evaluate polyprotic acid/base systems
 perform chemical calculations for polyprotic acid/base systems
Chapter 12:
 be familiar with the various types of titrations including those for strong
acids/bases, weak acids/bases, and polyprotic acids/bases
 use equilibrium chemistry to analyze acid/base titrations
 analyze a titration curve to deduce the quantities of acidic and basic
components in a mixture and what their pKa’s are
 use the Gran plot to determine titration end points
 be familiar with acid/base indicators and be able to pick appropriate indicators
for specific acid/base reactions
Chapter 13:
 demonstrate a clear understanding of complexometric tirations, specifically
EDTA titrations
 use equilibrium expressions to analyze complex formations
 perform EDTA titration calculations
 be familiar with metal ion indicators
Grading:
Class:
Lab**:
Total:
Homework assignments
4 - one hour exams (drop the lowest)
1 - final exam
11 lab reports
120 points
300 points
200 points
110 points
730 points
Extra Credit: During the semester I will offer problems totaling 25 points that may be
used to bring up your grade.
All exams MUST be taken during the scheduled time. The will be no makeup for missed
exams. In compliance with Lake Superior State University policy and equal access laws,
disability-related accommodations or services are available. Students who desire such
services are to meet with the professor in a timely manner, preferably the first week of
class, to discuss their disability-related needs. Students will not receive services until
they register with the Resource Center for Students with Disabilities (RCSD). Proper
registration will enable the RCSD to verify the disability and determine reasonable
academic accommodations. RCSD is located in South Hall Office 206. The telephone
number is (906) 635-2454.
**It is MANDATORY that you attend the laboratory. A failing grade in the
laboratory will result in a failing grade for the class.
Final Grade:
You MUST attend the lab. A failing grade in the laboratory will be an automatic failing
grade for the class. The final grade will be based upon the total points (840 points). The
letter grade given will be as follows:
Points
Letter Grade
681 to 730
A
657 to 680
A634 to 656
B+
613 to 633
B
584 to 612
B560 to 583
C+
540 to 559
C
511 to 539
C487 to 510
D+
465 to 486
D
438 to 464
D437 or less
F
Class Syllabus**
CH231 - Quantitative Analysis (Fall 2004)
Week of
Aug. 30, 2004
Sept. 8, 2004
Chapter/Topic
Chapters 1 & 2 Measurements & Tools of Trade
Chapter 3 – Experimental Error
Chapter 3 – Experimental Error
Sept. 13, 2004
Chapter 4 – Statistics and Spreadsheets
Sept. 20, 2004
Sept. 27, 2004
Chapter 5 – Calibration Methods
Exam 1 (Chapters 1 -5)
Chapter 27 – Gravimetric Analysis
Oct. 4, 2004
Chapter 6 – Chemical Equilibrium
Oct. 11, 2004
Oct. 18, 2004
Chapter 7- Let the Titrations Begin
Exam 2 (Chapters 27, 6 & 7)
Chapter 8 -Activity
Oct. 25, 2004
Chapter 9 – Systematic Treatment of Equilibrium
Nov. 1, 2004
Chapter 10 – Monoprotic Acid-Base Equilibria
Nov. 8, 2004
Exam 3 (Chapters 8, 9& 10)
Chapter 11- Polyprotic Acid-Base Equilibria
Chapter 11 – Polyprotic Acid-Base Equilibria
Chapter 12- Acid-Base Titrations
Chapter 12 – Acid-Base Titrations
Nov. 15, 2004
Nov. 22, 2004
Nov. 29, 2004
Dec. 6, 2004
Chapter 13 - EDTA Titrations
Exam 4 (Chapters 11, 12)
Chapter 13- EDTA Titrations
Dec. 13, 2004
Final Exam
**NOTE: The course syllabus represents the best estimate and projection of course
content, scope, and sequence. The syllabus is subject to change based upon the discretion
of the instructor.
Laboratory:
The laboratory is organized to allow the student experience in practical quantitative
analysis. Whenever possible, the laboratory methods will employ equipment and
practical techniques used in real world laboratories. Write ups for the specific laboratories
will be handed out one week in advance. The student is expected to attend the laboratory.
Additionally, the student is expected to maintain a professional laboratory notebook and
to prepare type written laboratory reports for each laboratory activity using the standard
format that is provided. The laboratory reports are due 7 days after the laboratory is
completed. Late reports will be accepted only upon permission from the instructor.
Scheduled Laboratories:
Week of:
Lab
Aug. 30
no lab
Sept. 13
Using Laboratory Apparatus
Sept 20
Gravimetric Determination of Chloride
Sept. 27
Gravimetric Determination of Iron as Fe2O3
Oct. 4
Preparation of Standard Acid and Base
Oct. 11
Analysis of a Mixture of Carbonate and Bicarbonate
Oct. 18
Kjeldahl Nitrogen Analysis
Oct. 25
Determination of Silver in an Alloy: Volhard’s Method
Nov. 1
Determination of Chloride in a Soluble Chloride: Fajan’s
Nov. 8
Determination of Water Hardness with EDTA
Nov 15
Analysis of Bleach by Iodometric Titration
Nov. 29
Analysis of an Iron Alloy or Ore by Titration with K2Cr2O7
Dec. 6
Check out
Standard Format for Laboratory Reports:
All reports should be typewritten with the exception of the raw data and calculations
which may be photocopied from your laboratory notebook and legibly written into the
report by hand, respectively. The report should adhere to the general outline below.
Depending upon the nature of the experiment, the laboratory instructor may also ask you
to include additional sections in your report or may ask you to delete a section of the
report.
Outline (Format)
I. Experiment Title, Date, and Your Name
II. Purpose of the Experiment (i.e., what is the experiment designed to do?)
III. Reaction Equations (when appropriate)
IV. General Description of the Experiment and the Observations
V. Raw Data (yellow carbon copies from laboratory notebook)
VI. Calculations (and Graphs if applicable)
VII. Final Results or Conclusions
Safety in the Laboratory
While working in the laboratory you are expected to comply with the safety rules which
follow, any and all rules posted in the laboratory or as established by your instructor.
Violations of the safety rules endanger both yourselves and other in the laboratory.
Students who violate the established rules and procedures may be subject to warnings,
reductions in grade, or expulsion from the lab. Safety rule violations include but are not
limited to the following:
1. Laboratory eye protection is required at all times in the laboratory. Not wearing
appropriate safety goggles for the activities assigned is a violation of the safety rules.
Note: Some activities such as pouring and mixing concentrated reagents require the
used of SPECIAL chemical splash goggles and perhaps other personal protective
equipment. Consult your laboratory instructor and always use the highest level of
protection available and appropriate for the task assigned.
2. Smoking, eating, or drinking in the laboratory is prohibited.
3. Pipetting by mouth or otherwise handling chemicals unsafely is prohibited.
4. Using an open flame to heat flammable liquids is prohibited.
5. Not working under a fume hood when directed to do so is a violation of
laboratory safety and subject to actions mentioned above.
6. Failing to report or clean up chemical spills or broken equipment is a violation
of laboratory safety and subject to actions mentioned above. Special spill kits are
available in the lab to handle a variety of spilled chemicals. Consult the laboratory
instructor for guidance using these kits.
7. Disposing of chemicals improperly. ALWAYS consult the instructor for the proper
handling instructions or location of the designated chemical waste container for the
experiment.
8. Working alone in the laboratory or working outside the regularly scheduled lab
times with the permission of the instructor is prohibited.
9. Performing unauthorized experiments or mixing unknown is prohibited.
10. Engaging in horseplay or other behavior that jeopardizes your safety or the
safety of others in the laboratory is prohibited.