|
B: LABORATORY
TIME: Monday, 12:00
pm-5:15pm
INSTRUCTOR: Issa I
Salame; office: J-1311
 :
(212) 650-6072
HOME
ASSIGNMENT: Before each lab read carefully the experiment description and
refer to the chapter in the text book dealing with the particular chemistry
content objectives
QUIZZES: Before each
laboratory starts the students will be asked to find an answer for one question
or solve the problem (15 minute quiz) dealing with the experiment which they are
about to do. The grading from quizzes will consist of 10 % of the total
laboratory grade.
Student are required to start their laboratory
experiments on time
ATTENDANCE:
You are required to come to the
lab on time. Attention: their will be a lateness penalty (10 points out of 100)
of you show up later than 1:15 p.m. Moreover, if you are late you will not get
your quiz points (10%). If you do not show up at all, your grade will be zero
PERFORMANCE:
 |
Always prepare for the
lab, so you can do the experiment efficiently. |
|
Handle the equipment and
chemical with care. Attention: safety glasses
must be worn while working with chemicals - you will not be allowed to
work if you do not bring them. |
|
Keep your workplace
clean |
|
Record the measurements,
calculations and results in a bind book. |
|
Before you leave the
lab, the instructor should see your results and sign there (you may
have to show the original results to the instructor later, so do not
lose your notebook). At that time ask any questions you have about
carrying out the calculations, doing the report, etc. |
REPORT:
The lab report should be typed or
hand written legibly on white 8.5 x 11 format paper and handed in to the
instructor on week after the experiment. Late reports will not be accepted.
The report should include:
|
Theoretical part (do not
write too much-it should not take more than one page) |
|
Experimental procedure |
|
Data analysis: detailed
calculations using significant figures and correct units. If there are
any graphs, they should also be included in this section. The graph
should be done using computer programs. If computer is not available,
graphs can be done on an accurate graph paper. In both cases linear
regression analysis is to be used to analyze data if linear dependence
is expected. |
|
Discussion: discuss your
results and analyze sources of errors that might have occurred during
your experiment. Explain how these errors could have been avoided. |
|
Answer to questions if
there were any. |
GRADING:
The lab grade carries 30% of the
final score. Each experiment is graded on the scale from 0 to 100 points.
| Quiz 10% |
| Performance in the class 10% |
| Form of the lab report 10% |
| Calculations 50% |
| Discussions 20% |
To arrange a make up of the lab a note from a
doctor, etc. HAS TO be shown.
SUGGESTED
TECHNIQUES:
|
Before
filling a pipette or burette always rinse it with small portions of
solution. |
|
In reading
meters and burettes, be careful to avoid parallax. |
|
Always read
your burette to the second decimal. |
|
Never weight
either a hot or a cold sample |
|
never put a
pipette into a bottle of stock reagents. You can contaminate the solution
and ruin every determination made with it. Instead, pour some of the
solution into a dry beaker and pipette from the beaker. Discard the
residue |
|
Use
graduated cylinder only for measuring approximate volumes |
SCHEDULE
OF LABORATORY EXERCISES
AND
CHEMISTRY CONTENT OBJECTIVES
DATE : Exercise
# TOPIC and chemistry content objectives
Jan. 29 1. Introduction to Mathcad; Introducing
how to use Mathcad to do:
| some basic computations |
| least square method |
| graphing |
| text editing |
Feb. 5 2. Applications of Statistics to
Data Treatment
| standard deviation |
| Gaussian distribution |
| Q-test |
| t-test |
Feb. 13 3. Determination of Iron in Ore;
|
standardization |
|
oxidation/reduction
reactions |
|
redox titration |
Feb. 26 4. Potentiometric titration of weak
monoprotic acid
|
acid/bases |
|
potentiometric titration |
|
end point |
|
acid dissociation
constant |
|
calibration of pH meter |
March 5 5. Study of diprotic acid equilibria
by potentiometric titration
|
acid/base titration |
|
potentiometric titration |
|
end point interpretation |
|
chemical equilibrium |
| acidity constant |
March 12 6. Constructing binding curve:
dealing with theory and experimental data
|
acid/base titration |
|
chemical equilibria |
|
complex systems |
|
binding curve |
*********************** ROTATION
STARTS
(each group will obtain an
individual schedule)
7
Determination of calcium in calcium gluconate
| analysis of metal content |
| properties of EDTA |
| complex formation constant |
| EDTA titration |
8
Complex-formation titration: determination of chloride
|
precipitation |
|
solubility |
|
Argenometry |
|
complex formation |
9
Coulometric determination of Vitamin C (ascorbic acid)
|
oxidation/reduction
reactions |
|
coulometry |
10
Spectroscopic Determination of the pKa of an acid/base Indicator
|
chemical equilibrium |
|
acids and bases |
|
dissociation of
indicators |
|
spectrophotometry |
|
absorbance |
11
Determination of manganese in steel
|
spectroscopy |
|
absorbance |
|
Beers Law |
| oxidation/reduction |
12 Analysis
of organic acids in fruit juice by reversed phase HPLC
|
liquid chromatography |
|
column efficiency |
|
the principles of
chromatographic separation |
|
calculation of
concentration based on calibration curves |
Make-up
Check out
created
by TJB. last
updated: December 17, 2008 updated
by Thiri
| 
