Organic Chemistry II Laboratory

Course Objectives

This course is meant to re-enforce some of the organic chemistry concepts in CHEM 224, especially characteristic reactions used in identifying the different functional groups in organic chemistry. Demonstrations on physical and chemical experimental methods used to identify organic compounds and some reactions that would synthesize some organic compounds

Learning Outcomes

At the end of this course, students

  • Would be able to perform many practical chemical techniques. 
  • Should have a better understanding of the preliminary laboratory techniques of organic chemistry.
  • Should be able to identify organic compounds by physical and chemical experimental methods.
  • Would have developed some experimental skills and research potentials
Assessment and Grading

To satisfy part of the requirement for this course, attendance and participation in all laboratory sessions is mandatory. Assessment would be based on grades from Laboratory assignments (60 points), Lab exam I (20 points) and Lab exam II (20 points).


The labs will be given to students as assignments. Experimental data will be provided for analysis, from which students can make deductions and arrive at conclusions. These will be submitted via turn-it-in in the assignment folder on MyCourses. 

Each lab assignments (labs 2 – 9) will be graded to a total of 10 points per lab.

Best six of eight assignments will count towards final grade: 6 x 10: Total of 60 points from assignments.

Lab Exam 1 (MCQs on ExamSoft) from labs 1 – 5: Total of 20 points.

Lab Exam 2 (MCQs on ExamSoft) from labs 6 – 9: Total of 20 points.

Students cannot re-do the labs that they have missed.


SAS Grading Scale:  Grades will be assigned as follows:

A = 89.5% or better

B+ = 84.5 - 89.4%

B = 79.5 - 84.4%

C+ = 74.5 - 79.4%

C = 69.5 - 74.4%

D  = 64.5 - 69.4%

Laboratory Sessions:
  • Lab Session #1: Introduction & Lab Safety
  • Lab Session #2: Melting point determination
  • Lab Session #3: Reactions of Alcohols and Phenols
  • Lab Session #4: Formation of Ester (Preparation of Ethyl acetate)
  • Lab Session #5: Qualitative tests for Aldehydes and Ketones
  • Lab Session #6: Determination of an unknown carboxylic acid
  • Lab Session #7: Reactions of Amines and carboxylic acid Lab Session #8: Titration of an amino acid (glycine)
  • Lab Session #9: Isolation of Caffeine from team

Lab #1: Introduction and Safety

Students will be introduced to this course content, delivery, and expectations. There will be a discussion on laboratory safety procedures and considerations 

Laboratory Safety:

  1. A laboratory coat must always be worn in the lab. This will protect you and your clothes from any contaminants that may be used during the laboratory experiments.
  2. Shoes must have closed toes and heals. NO SLIPPERS, NO FLIP-FLOPS, NO SANDALS. You may be asked to leave if you are not dressed properly to conduct an experiment.
  3. In general, gloves should be worn during the lab exercises. These will protect your skin from corrosive chemicals. Gloves are NOT worn outside the lab. You do not wear gloves to go to the bathroom, to handle doorknobs, do not handle your pen, do not scratch your face... 
  4. NEVER pipette solutions with your mouth, eat, drink, smoke or apply cosmetics in the lab.
  5. NEVER pour any chemical or solution into a sink without authorization. 
  6.  NEVER use flames with or near volatile solvents 
  7. NEVER return reagents to stock bottles. 
  8. NEVER smell specimens or chemicals directly. 
  9. Use caution when using equipment for heating or melting reagents (e.g. Boiling water baths).
  10. ALWAYS report any spillage or accident, however minor, to your instructor
  11. Wash hands thoroughly with soap and water after handling laboratory reagents and especially prior to leaving the laboratory when the session is completed.

N.B: Your Instructor may decide to modify an experiment, change the reagents or change the concentration of reagents based on logistics and experimental trial runs. It is your responsibility to pay attention to detailed instructions for any such modifications during the lab sessions.

LAB 2: Determination of the Melting Point of a Solid Substance.

Aim:  To determine the melting point of given solid substance.

Theory: The change in the state of a compound from solid to liquid when it is heated is called melting, and the temperature at which a solid in its pure form melts is called the melting point. At the melting point, the solid and liquid exist in equilibrium. The melting point of a substance depends on pressure and is usually specified at a standard pressure. 

Every pure solid has a characteristics melting point therefore determination of melting point helps in identification of the compound. Presence of impurities lowers the melting point of the solid. Thus, Melting point also serves as a criterion of purity of a compound.

Materials required: Given solid organic compound, Thin walled capillary tubes   (8 – 10 cm in length and 2 mm in diameter), Paraffin oil, Laboratory thermometer, Heating medium (Hot plate), magnetic stirrer, 500ml beaker, retort stand, and rubber band


  1. Take a fine capillary of length 5-6cm. seal its one end by inserting the end of the capillary tube horizontally into the extreme edge of a small steady Bunsen flame for a few seconds, rotating the capillary meanwhile.
  2. Take a small quantity of the compound whose melting point is to be determined on a porous plate and powder it with a spatula.
  3. Introduce the powdered compound in the capillary tube by introducing the open end of the capillary tube into the powdered compound and gently rotating it. Gently tap the capillary tube against the porous plate so that the compound sinks into the closed end. Repeat the procedure of introducing and tapping three to four times.
  4. Moisten the bulb of thermometer with liquid paraffin and attach the capillary to the lower end of the thermometer.
  5. Place the thermometer with the capillary tube in the melting point apparatus containing at least two third of its volume liquid paraffin in such a way that the closed end of the capillary remains below the surface of Liquid paraffin (See fig 1 below)
  6. Now heat the beaker gently and note down the temperature from time to time and finally note down the temperature (t 0C) at which the compound starts melting (t1 0C) and completely melts (t2 0C).
  7. Repeat the experiment with a new capillary tube and fresh quantity of the substance.



        Fig1: Set up of the apparatus for melting point experiment



Melting points

  1. t1 =  _______________ 0C
  2. t2 =  _______________  0C

Mean Melting point = (t1+t2)/2 0C


  1. Use dry and powdered sample for the determination of melting point.
  2. Packing of the powder should be uniform without any big air gaps between the solid particles 
  3. The capillary tube should be filled one fifth of its length.
  4. Maintain uniform temperature of the liquid bath.
  5. The rate of heating should be controlled. It should be very slow near the melting point so that the melting point can be recorded accurately.


Assume that the compound provided has a melting point of 80oC, and you got 75oC after your experiment, what conclusions can you make about the compound?

LAB 3: Reactions of Alcohols and Phenols

AIM: To observe the reactions of some alcohols and phenols

Principle: Based on the physical and chemical characteristics of alcohols and phenols

Materials required: 10ml each of Ethanol (A), Butan-2-ol (B), 2-methyl butan-2ol (C), and unknown D. Phenol (2g), 20 test tubes, 1% soln. of Sodium dichromate, Glacial ethanoic acid, Conc. H2SO4, Conc. HCl, 5% Iron (III) chloride solution, iodine solution, sodium hydroxide and water bath set at 60oC..


  1. Sodium dichromate is a toxic compound. The use of plastic gloves is mandatory.
  2. Conc. HCl and H2SO4 are very corrosive and most be handled with utmost care
  3. Observe all other laboratory safety precautions


  • Present results for the reaction of each test reagent as shown in tables below.
  • Perform tests a, b, c, on alcohols A, and the unknown provided. 
  • To distinguish the various types alcohols, perform tests d and e on all the alcohols provided including the unknown.
  • Perform tests f, g, and h on phenol.
  • Write equations for tests b, c, d, e, g and h. 




a) Solubility

Test the solubility of alcohol, by taking about 1ml of alcohol in a test tube and adding an equal amount of water. Dip litmus paper in the resulting solution and note any change







b) Ignition

Place a about 1ml of the alcohol in a crucible and ignite (Write equation for combustion of butanol







c). Esterification

To about 2 cm3 of alcohol, add about 1 cm3 of glacial ethanoic acid followed by a few drops of concentrated sulfuric acid.

Heat the mixture in a water bath.

Pour the resulting mixture into water and note the smell

Write equation for esterification of ethanol with ethanoic acid







 d) Oxidation

To each of the four test tubes provided, add 2mls of a 1%      sodium dichromate solution and 5 drops of conc. Sulfuric acid and mix the contents thoroughly. Add 10 drops of A in tube 1, 10 drops of B in tube 2, 10 drops of C in tube 3 and 10 drops of your unknown to the fourth tube. 

Cork all 4 test tubes and warm gently in a 40 – 50oC water bath for a minute. Observe and record any color changes.






e) Triodomethane (Iodoform) test

Add about 5 cm3 each of iodine into two test tubes. Then add 5 drops of ethanol to one tube and 5 drops of  Propan -1- ol into the other.

Now add sodium hydroxide carefully until the iodine color has almost discharged and warm the mixture in a water bath for 2-3 minutes. (The temperature should not exceed 60C). Cool the tube and note the crystals formed.Write the equation for the formation of CHI3 (Iodoform reaction)






f) Solubility of phenol

Take enough phenol to cover the bottom of a test tube and add about 2 cm3 of water. Stopper the test tube and shake to obtain an emulsion. Remove the cork, place the test tube in a beaker of water and warm. Put a thermometer in the phenol solution and note the temperature when the emulsion clears. Test also the solution with litmus paper.

Cool this solution and use for other tests






g) Sodium hydroxide

To 5 drops of aqueous phenol, add sodium hydroxide until a clear solution is obtained. 

Add a few drops of concentrated hydrochloric acid and note the reappearance of Phenol






h) Iron (III) chloride

To a solution of phenol add 1 drop of iron (III) chloride






AIM: To prepare and purify ethyl acetate

THEORY: Esters frequently have distinctive odors and are found in the flavorings of many fruits and plants. An ester is a chemical compound that is formed when an organic acid reacts with an alcohol. Concentrated sulfuric acid, H2SO4, can be used to catalyze the reaction. Concentrated sulfuric acid is a strong dehydrating agent and helps the reaction by removing the water molecules as they are formed.

  • If acetic acid and ethanol are reacted, the reaction shown below occurs.


The product is called ethyl acetate. The systematic name for acetic acid is ethanoic acid, and the product is also known as ethyl ethanoate.

In this experiment we will prepare the ester known as ethyl acetate (ethyl ethanoate) and purify it by distillation.


  • Acetic acid, concentrated, 17.4 M (glacial)
  • Ethanol (ethyl alcohol, denatured alcohol)
  • Sulfuric acid, concentrated (18M)


Erlenmeyer flask, 125-mL (2)             

Boiling stones or glass beads


Distilling flask



Beaker, 400-mL for water bath 

Bunsen burner, ring & wire gauze

Measuring cylinder                             

Capillary dropper

Safety Precautions!

  • Wear Chemical Splash Goggles and a Chemical-Resistant Apron.
  • The concentrated sulfuric acid used is very hazardous. In case of accidental spillage, wash spills off yourself immediately with large amounts of water. Neutralize spills on the laboratory bench with baking soda.
  • The organic acids and alcohols are flammable. Use great care around flames. Do not heat directly with a burner but use a water bath.
  • The alcohols are all poisons. Do not ingest them. Wash yourself with soap and water if you spill some on yourself.


Preparation of purification of ethyl acetate (ethyl ethanoate).

  1. Preparation of ethyl acetate.


Diagram: Showing set up of apparatus for preparation of ethyl acetate

  • In one 125-mL Erlenmeyer flask, place 10-mL ethanol, 12 mL glacial acetic acid, 15 drops of concentrated sulfuric acid (18 M), and a boiling stone. 
  • The condenser should be clamped in a vertical position, with the bottom of the condenser inside the flask. When the condenser is inserted in this manner it acts as a reflux condenser, allowing the vapors of the mixture to condense and return to the reaction vessel. 
  • Slowly run cold water through the condenser, in at the bottom and out at the top. Heat the flask in a hot water bath. 
  • Raise the temperature of the hot water until the mixture in the Erlenmeyer flask is gently boiling and continue heating for about 15 minutes. 
  • Cool the mixture.
  1. Distillation of ethyl acetate.



Diagram: Showing set up of apparatus for distillation of ethyl acetate

  • Pour the mixture (including the boiling stone) into a distilling flask and connect the condenser to the side arm of the flask. 
  • Insert a thermometer. 
  • Heat the bottom of the distilling flask in a hot water bath until no more distillate is coming over. 
  • Record the temperature at which the distillation begins and the temperatures during and at the end of distillation. 
  • Look up the boiling point of ethyl acetate and compare to the distillation temperature.


1 Write the equation for the formation of ethyl acetate     2 What is the purpose of sulfuric acid?

  1. What happens if water is removed from the reaction mixture.            
  2. Write the structure of the product formed when ethanol is oxidized by  sodium dichromate

LAB #5: Qualitative tests for aldehydes and ketones

Aim: To distinguish between Aldehydes and Ketones.

Principle: Both aldehydes and ketones contain the carbonyl group, and both undergo nucleophilic addition reactions, with nucleophiles.

However, while aldehydes are easily oxidized to yield carboxylic acids,

RCHO → RCO2H, ketones are unreactive toward oxidation. This reactivity difference is a consequence of structure: aldehydes have a (CHO) proton that can be removed during oxidation, but ketones do not. In other words, Aldehydes can be oxidized (Removal of hydrogen from it), because the carbon of the carbonyl group has hydrogen attached to it. Ketones have none. Compounds which are oxidized act as reducing agents.

Aldehydes can be distinguished from ketones by their reaction towards the following mild oxidizing agents:


Experiments should be carried out and results presented as indicated below:




1). Place 2ml of a 5% AgNO3 soln. in a freshly cleaned test tube. Add 5% NaOH soln. dropwise until a black ppt forms.

Dissolve the ppt by adding dropwise with stirring NH4OH until the soln. just becomes clear. Avoid adding excess ammonia. Divide the soln. into three parts. Add 10-15 drops of the compounds to be tested to each of the parts. Cork and heat for about

1 minute in a 60oC water bath. Record your result.



2). Mix 5 ml of Fehling’s solution A with 5 ml of Fehling’s soln. B in a test tube. Divide the resulting soln. into three parts and add 1 ml of each of the compound to be tested to each of the parts. Cork the three test tubes place them on a 60oC water bath and heat for about 10 mins.

A positive test is indicated by a change in the blue colour of the solution and the slow formation of a fine brick red CU2O ppt.

Record your result.



3). To each of 3 test tubes, add 2 ml of a 1% Sodium dichromate solution and 5 drops of conc. Sulfuric acid. Mix the content thoroughly. Add 10 drops each of the compounds to be tested.

Cork the test tubes and warm gently in a 40 – 50oC water bath for a minute.

Observe and record any color changes.




LAB #6: Determination of an unknown carboxylic acid

Aim: To determine the molar mass of an unknown monoprotic carboxylic acid by titration and hence identify the acid. 


Principle: At the equivalence point of the titration, the moles of OH (base) are equivalent to the moles of H+ (acid) in the sample. The moles of OH added to the solution from a burette are calculated from the concentration of the base (MOH) and the volume of base (VOH) added, as:


Because it is a monoprotic acid, the moles of acid are equal to the moles of OH at the endpoint of the titration.


The units of molar mass are g/mol. This intensive property is the ratio of two extensive properties, as is shown in the figure below.

The lab goal is to determine the molar mass of an unknown monoprotic acid. The grams of acid are determined from weighing the acid and the moles are determined from the titration with NaOH. 

Materials required: Weighing balance, Burette, Pipette, Erlenmeyer flasks (3), Methanol (30mls), 0.1M NaOH (150mls), 0.15g of an unknown carboxylic acid (Benzoic acid) and phenolphthalein indicator.


1). Accurately weigh 0.15g of your unknown acid and transfer it into a 125ml Erlenmeyer flask. Add 10 ml of methanol and 2 drops of phenolphthalein indicator and swirl the contents to ensure proper mixing.

2). Titrate against a standardized 0.1M NaOH solution. The change in color from colorless to pink can be noted once the equivalent point has been reached. Record your readings.

3). Repeat the titration with a new weighed sample of the same carboxylic acid. The mass used for the second titration should be different from the mass used for the first determination. 

Calculate the molar mass (g/mol) The two values should agree within ±2 amu. If they do not, perform a third titration.

4). Wash the burette after the last titration, while still clamped. Drain the burette, then slowly add about 10 mls of water and drain; then 10mls of dil. HCl and drain; finally add 50ml of distilled water and drain.

Do not place the burette under the faucet in order to wash it 

5). Identify your unknown carboxylic acid by matching your results with the possibilities listed in the table provided


Tabulate your results as shown below:


Attempt #1

Attempt #2

Attempt #3

 Mass of Carboxylic acid




 Final burette reading




 Initial burette reading




Volume of NaOH needed for neutralization




Molarity of NaOH (Standardized)




 Molar mass of the acid




 Average Molar mass of unknown




Conclusion: My unknown carboxylic acid is -------- Suggest a molecular formula for this acid: 

How many carboxylic acids with this formula are possible?

LAB #7: Reactions of Amines and Carboxylic acids

AIM: To test and observe the reactions of some amines and carboxylic acids.


  • Phenylamine (Avoid skin contact. Toxic & harmful because of skin absorption)
  • Ethanoic acid
  • Red litmus paper
  • Sodium nitrite (10%)
  • Hydrochloric acid (Conc), 5% and 10% HCl
  • Propanol
  • Sodium hydroxide
  • Sodium carbonate salt (about 0.5g)
  • Lime water
  • Benzene sulphonyl chloride


Experiments to be carried out and recorded as shown below:




a) Solubility in water

Test the solubility of phenylamine in water by shaking 3 drops of phenylamine with 2cm3 of water. Dip a piece of red litmus paper inside and observe any color change.



b) Solubility in HCl

Test the solubility of phenylamine in HCl



by shaking 3 drops of phenylamine with  2cm3 of HCl. Compare with sol. In water






c) Nitrous acid test 

Cool a mixture of sodium nitrite and a solution of the amine in and ice bath. The mixture must be added in the ice bath. 

Add moderately concentrated hydrochloric acid to the mixture above in the ice bath. Note the effervescence.

All additions for reaction c must be done in the ice bath.






d). Hinsberg test  

Place about 10-15 drops of the amine

(0.5 – 0.8 g ,if solid) in a test tube. Add 15 drops of benzenesulphonyl chloride and 10 – 15 drops of 10% NaOH solution. Stopper the test tube and shake it vigorously for a few mins. Remove the stopper and warm the test tube in a water bath (60 – 70 0C)  for about 1-2 mins and check for reaction. If ppt. forms in the alkaline solution, add 3-5 ml of a 10% and shake the test tube. If the alkaline solution is clear,



acidify it with a 10% HCl to see if a ppt  will be formed.






d) Add ethanoic acid to propanol






e)Add ethanoic acid to sodium hydroxide






e) Add ethanoic acid to sodium carbonate and test the gas given off with lime water. ​​​​​​​




AIM: To study the titration curve of an amino acid (glycine).

Theory: Titration curves are obtained when the pH of given volume of a sample solution varies after successive addition of acid or alkali. The curves are usually plot of pH versus the volume of titrant added.

Amino acids are amphoteric molecules which can be titrated either against an acid or an alkali. They are weak Polyprotic Acids which exist as zwitterions at neutral pH. When an aqueous solution of an amino acid is titrated with an acid, it acts as a base, with a base, it acts as an acid.

In this experiment we are finding out the titration curve of the amino acid Glycine.


Glycine is a diprotic amino acid which means that it has two dissociable Protons, one on the α amino group and the other on the carboxyl group. In this fully protonated form; it can donate two protons during its complete titration with a base.  In the case of Glycine, the R group does not contribute a dissociable Proton.


The dissociation of proton proceeds in a certain order which depends on the acidity of the proton: the one which is most acidic and having a lower pKa will dissociate first.  So, the H+ on the α-COOH group (pKa1) will dissociate before that on the αNH3 group (pKa2).


0.1M Glycine

0.1M NaOH


pH meter

250ml conical flask

5ml pipette


Observe all laboratory precautions


Pipette 25 cm3 of glycine into the conical flask provided and measure the pH. Now fill the burette to the zero mark with 0.1M NaOH. Using the burette, add 5ml of 0.1M NaOH to 25cm3 of glycine and record the pH of the resulting solution. Continue adding 5 ml of NaOH at a time and measure the pH for every 5ml added. Record your results as shown in the table below.


Volume of NaOH added

Total volume of NaOH 

pH of solution






































  1. Using the data collected, draw a titration curve with pH on the vertical axis [shorter axis] and the volume of NaOH added on the horizontal             axis [longer axis].
  2. What is the mathematical relationship between pKa and PI      
  3. Obtain the value of pI (isoelectric point) from the graph. 
  4. What is a zwitterion?
  5. Draw the structure of glycine and state why glycine is unique compared to the other amino acids.


AIM: To demonstrate the isolation of a natural product from a biological source, using extraction techniques.


Extraction with a solvent (Solvent extraction) is a separation technique most frequently employed to isolate one or more components of a mixture. The technique is based on the preferential solubilities of the components of the mixture for two different immiscible solvents. 

It involves the partial removal of a solute from one liquid in which it is less soluble to another immiscible liquid in which it is more soluble. In most cases, an organic solvent is used to remove an organic solute from an aqueous solution or suspension. If a solute is shaken with a mixture of two immiscible solvents at a fixed temperature, the solute will distribute itself in both solvents according to its solubility in each. The solute will partition itself according to the ratio:

Kp = [solute]A/[solute]B

Where Kp is the distribution coefficient, [solute]A is the concentration of the solute (in moles/L) in solvent A (usually the organic solvent) and [solute]B is the concentration of solute in (in moles/L) in solvent B (usually water).

For example, 6.67g of phenol is dissolved in 100ml of water, while 8.33g will dissolve in 100ml of benzene, the distribution coefficient will be:

Kp = (8.33g/100mL)benzene /(6.67g/100mL)water =1.25

Solvent extraction is more efficient if a certain volume of the extracting solvent is used in several portions rather than one.

Caffeine is an alkaloid that is present in coffee, tea, cola, chocolate any many nonprescription drugs. 

Caffeine is soluble in water because it has several polar and basic functional groups. 


This property makes it insoluble in aqueous base. Thus, by adding a weak base (e.g. sodium or calcium carbonate) to an aqueous solution of tea extract, one can decrease its solubility in water  and increase its solubility in a less polar organic solvent ( such as CH2Cl2), into which the caffeine can be easily extracted, using a separatory funnel. Any neutral compound will be extracted into the organic phase, but unfortunately, there are a few of these present in tea. Any acidic compounds (such as tannic acid, a major component of tea) will be deprotonated and will remain in the aqueous phase.

Therefore, Sodium carbonate serves two main functions: to place caffeine in a more basic environment so that it has a higher affinity for dichloromethane and to  cause the tannins which are acidic to form phenolic salts in the aqueous solution.


Observe all laboratory precautions.


  1. In a 400mL beaker, place 10 tea bags and approximately 100mL of water. Bring to boil on the hot plate and continue to boil for about 15 minutes.
  2. Carefully remove the beaker from the hotplate, remove and discard the teabags, and dissolve 15g of Na2CO3 in the tea solution by stirring 
  3. Cool the tea solution in and ice water bath, then transfer it into a separatory funnel, using a funnel.
  4. Add 20mL of methylene chloride via a funnel and shake the mixture gently. DO not shake to vigorously, or you will get an emulsion (i.e. a mixture consisting of droplets of one phase suspended into the other). If this happen let it stand for about 15 minutes to allow separation of the layers.
  5. Extract the aqueous layer with another 20mL portion of methylene chloride
  6. Combine the organic extracts in a 125mL conical flask, and dry them with about 1g of anhydrous MgSO4
  7. Allow the solution to stand for about 10 minutes, swirling it occasionally to complete the drying.
  8. Keep the aqueous phase in a beaker – do not discard until you are sure you do not need it anymore
  9. Gravity-filter the methylene chloride solution into a small pre-weighed beaker. Add one boiling chip, and carefully evaporate the solvent to dryness in a hot water bath or a large beaker of water on a hotplate in the hood.
  10. Remove the boiling chip, reweigh the beaker, and calculate the yield of crude caffeine


  1. Tea contains approximately 2% caffeine by weight. Assume that you started with 25g of tea leaves, calculate the percentage yield of your crude extract.
  2. Suppose you forgot to add sodium carbonate to the tea solution prior to extraction.  What effect would this have on your yield?
  3. What are the advantages and disadvantages of using ether in solvent extraction?
  4. Why was the extraction with methylene chloride done twice with 20mL each time, instead of once with 40mL of methylene chloride?
  5. Write equations for the reactions between ethanol and Na, phenol and NaOH and between ethanoic acid and Na2CO3.

CHEM 225 Laboratory Schedule – Spring 2022








Introduction/Lab Safety




Determination of the melting point of an organic compound.




Reactions of alcohols and phenol



Feb 07 - 11

NO Labs




Qualitative tests for Aldehydes and Ketones




Formation of ester (Preparation of Ethyl acetate)




Lab Exam 1



Mar 07 - 11

Midterm Week (No Labs)




Determination of an unknown carboxylic acid




Reactions of Amines and carboxylic acid




Titration of an amino acid (glycine)



Apr 04 - 06

No Labs




Isolation of Caffeine from tea.




Lab Exam 2







May 02 – 06

Final Exam Week (No Labs)

School of Arts and Sciences Master Syllabi — Info for All Sections

Plagiarism Policy

Academic Integrity

The St. George’s University Student Manual (2019/2020) states as follows:

Plagiarism is regarded as a cardinal offense in academia because it constitutes theft of the work of someone else, which is then purported as the original work of the plagiarist. Plagiarism draws into disrepute the credibility of the Institution, its faculty, and students; therefore, it is not tolerated” (p. 48).

Plagiarism also includes the unintentional copying or false accreditation of work, so double check your assignments BEFORE you hand them in.

Be sure to do good, honest work, credit your sources and reference accordingly and adhere to the University’s Honor Code. Plagiarism and cheating will be dealt with very seriously following the university’s policies on Plagiarism as outlined in the Student Manual.

Your work may be subject to submission to plagiarism detection software, submission to this system means that your work automatically becomes part of that database and can be compared with the work of your classmates.

Attendance Requirement

The St. George’s University Student Manual (2019/2020) states as follows:

Students are expected to attend all classes and or clinical rotations for which they have registered. Although attendance may not be recorded at every academic activity, attendance may be taken randomly. Students’ absence may adversely affect their academic status as specified in the grading policy. If absence from individual classes, examinations, and activities, or from the University itself is anticipated, or occurs spontaneously due to illness or other extenuating circumstances, proper notification procedures must be followed. A particular course may define additional policies regarding specific attendance or participation” (p. 9).

Examination Attendance

The St. George’s University Student Manual (2019/2020) states as follows:

All matriculated students are expected to attend all assigned academic activities for each course currently registered. Medical excuses will be based on self-reporting by students. Students who feel they are too sick to take an examination or other required activity on a specific day must submit the online SAS medical excuse, which is available on Carenage. Students are only allowed two such excuses a year. Upon consultation with the Director of University Health Service, the third excuse will result in a mandatory medical leave of absence. The policies regarding make-up examinations are at the option of the Course Director” (p.46).

For additional specific examination policies and procedures, refer to the St. George’s University Student Manual (2019/2020), pages 31 through 37.

Student Accessibility and Accommodation Services Policy

The St. George’s University Student Manual (2019/2020) states as follows:

A student with a disability or disabling condition that affects one or more major life activities, who would like to request an accommodation, must submit a completed application form and supporting documentation to the Student Accessibility and Accommodation Services (SAAS) located in the Dean of Students Office. It is highly recommended that students applying for accommodations do so at least one month before classes begin to allow for a more efficient and timely consideration of the request. If a fully completed application is not submitted in a timely fashion, an eligibility determination may not be made, and accommodations, where applicable, may not be granted prior to the commencement of classes and/or examinations” (p. 8).


It is the responsibility of the student to read and understand the policies, laws, rules and procedures that while they could affect your grade for a course, have not been specifically outlined in the course syllabus. These are contained in the St. George’s University Student Manual.