Acetaminophen Lab Report
Acetaminophen Lab Report
Acetaminophen Lab Report
Recrystallization Techniques
Armaan Gill
20777133
Partner: Brittney Persad
TA: Yuxing
Experiment Performed: November 6, 2018
CHEM 120L Section 009
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Introduction
The objective of this experiment was to retrieve a crude and pure product of
acetaminophen, and determine the melting point ranges of both products. The main purpose of
technique. Acetaminophen is an organic medicinal drug which aids in relieving pain and
reducing fevers. This drug is created by reacting p-aminophenol with acetic anhydride to produce
acetaminophen and acetic acid. The amine group of p-aminophenol is acetylated by acetic
anhydride to construct an amide group. This results in acetic acid being one of the by–products.
After this reaction takes place, acetaminophen is precipitated out of solution due to the solubility
of the products. Acetic acid is highly soluble whereas acetaminophen is highly insoluble in
water, which results in the two products separating and acetaminophen solid forming. In this
experiment, the vacuum filtration, and recrystallization techniques are utilized along with warm
and cool water baths to aid in reactions. The warm water bath was used to dissolve the
crude/pure product in its solvent, distilled water. The ice water bath was used to allow the
crude/pure product to precipitate out of the solution. The vacuum filtration technique filters out
all of the acetic acid, leaving the solid crude or pure product. A sample of both the crude and
pure product are collected to determine their melting temperature ranges. Theoretically, the crude
product should have a lower melting temperature then the pure product due to the fact that the
crude product is less pure. This means the crude product contains more foreign elements to the
precipitate which lowers the energy within its bonds. A pure product has stronger bonds than an
Procedure
The experimental procedure used for this experiment was outlined in CHEM 120L lab manual,
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Experimental Observations
Stage Observations
Round bottom flask -3.24 grams p-aminophenol and 10 mL deionized water heated at 70oC
(warm bath) -4.00 mL pure acetic anhydride added, giving the solution a yellow color,
and continued heating
-All p-aminophenol dissolved 6 minutes after pure acetic anhydride added
-Solution cooled at room temperature for 10 minutes while stirring
Round bottom flask -Yellow solution cooled for 15 minutes
(ice-water bath) -White precipitate formed at the bottom of flask
Vacuum filtration -Solid kept under vacuum for 5 minutes
(crude product) -Aqueous solution filtered out
-3.92 grams of white powdery substance (crude product) obtained
Recrystallization -3.92 grams of crude product and 39.2 mL of deionized water added to
(warm water bath) Erlenmeyer flask
-Mixture heated till dissolved then cooled at room temperature
Recrystallization -Clear solution cooled for 10 minutes
(ice-water bath) -White substance recrystallized at bottom of flask
Vacuum filtration -Solid kept under vacuum for 5 minutes
(pure product) -Aqueous solution filtered out
-3.44 grams of shiny white powdery substance (pure product) obtained
Melting -Product started melting at 163oC
temperature for -Product finished melting at 165oC
crude product
Melting -Product started melting at 163oC
temperature for -Product finished melting at 168oC
pure product
Percent Yield:
% Yeild = Actual Yield – Theoretical Yield x 100%
Theoretical Yield
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Discussion
In this experiment, a p-aminophenol was taken through a series of reactions to ultimately
form a pure product of acetaminophen. This experiment accomplished the production of the
crude product, the pure product, and from these two products, the melting temperature ranges of
each were measured. From 3.24 grams of p-aminophenol, 3.92 grams of crude product was
produced and 3.44 grams of pure product was produced. The melting temperature range of the
crude product was 163oC to 165oC and the pure product was 163oC to 168oC. The accepted value
of the melting temperature of acetaminophen is 169 oC to 170oC. (NIST, 2018). The experimental
temperature range of the pure acetaminophen was only a few degrees below the accepted
temperature range. This means that the experiment was extremely effective and efficient as the
accepted temperature range is for a purified acetaminophen. However, even though the
acetaminophen in the experiment was a pure product, it was not completely pure. There was a
percent error of 23.4% which means that the pure product obtained was not 100% pure. This
error could have been the cause of some of the acetaminophen remaining dissolved in the
solution separated from the precipitate. As predicted, the purer substance has a higher melting
temperature than an impure version of the same substance. Since the pure product produced in
the experiment was not completely pure, it resulted in a temperature range lower than the
expected. However, the temperature range was extremely close which means the experiment was
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Questions
1. In this experiment crude acetaminophen was purified using the technique of
recrystallization; answer the following questions regarding this technique:
a. What could happen if 5 mL of water was added for every 1 g of crude product?
Adding 10 mL of water per every 1 g of crude product was instructed because this would result
in a saturated solution where no more solute can dissolve. If 5 mL of water was used instead, it
would have resulted in a supersaturated solution where there is a much higher solute
concentration than the solvent which could possibly lead to the formation of some crystals.
b. What could happen if 15 mL of water was added for every 1 g of crude product?
If 15 mL of water was used for every 1 g of crude product, the solution would have become
unsaturated where more solute can dissolve. Adding 10 mL or 15 mL may give you the same
results because if the solute can dissolve in 10 mL, it can also dissolve in 15 mL. In this case, the
c. Cold solvent was used to aid in the transfer of the recrystallized product. What could
happen if room temperature solvent was used?
Higher temperatures result in a higher rate of dissolving as the molecules begin to move faster
with more energy. Since room temperature is higher than the temperature of the cold solvent,
some of the recrystallized product could have dissolved due to the warmer room temperature.
d. What is the purpose of scratching the inner walls of the round bottom flask?
This causes small particles of glass from the flask to get scratched off and react with the solution
as nuclei for crystal growth. The glass particles act as a seed allowing crystals to form around the
seed from the dissolved solution. This induces crystallization in the solution.
2. How is measuring the melting points of your samples help to assess the purity?
An impure sample melts faster than a pure sample due to the impurities in the structure of the
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solid. A pure substance has more tightly packed molecules than an impure substance. This fact
means that the pure substance requires more energy to break apart the bonds between molecules
than an impure substance. This allows the impure substances to have lower melting temperatures
than the pure substances as less energy is required. That is also the result achieved in the
experiment, the pure product had a higher melting temperature than the crude product.
3. Research a product a product (other than acetaminophen) that is created using organic
synthesis. Write a short paragraph (200 words or less) summarizing your research. Some
things to think about: What product is synthesized? What are the reagents used? What is
the process of synthesis? How has this product changed the world we live in?
One product produced using organic synthesis is aspirin. The two main reagents used to
create this product were salicylic acid and acetic anhydride. (Olmsted, 1998). The products of
this synthesis reaction are acetylsalicylic acid (aspirin) and acetic acid. Acetic acid is highly
soluble and acetylsalicylic acid is highly insoluble. This causes the aspirin to simply precipitate
Aspirin has changed the world by being one of the many drugs that aid to reduce fever and
act as a pain killer. Salicylic acid, one of the ingredients of making aspirin, it is used to create a
variety of products using organic synthesis as it is a plant hormone. (Olmsted, 1998). Relative to
health treatment, salicylic acid comes from willow bark which is another reagent that is a
headache remedy. Salicylic acid has similar functions to aspirin except is much easier for the
body to consume.
4. Find one organic amine (other than p-Aminophenol) and one organic amide (other than
acetaminophen), draw the structure for each and clearly indicate the amine/amide group.
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Conclusion
The main objectives of this experiment consisted of creating a crude product of
acetaminophen, and then using that to create a pure product. Another objective of this experiment
was to determine the temperature ranges of each, crude and pure product. The objectives
regarding this experiment were achieved as the crude and pure products were produced and the
melting temperature ranges were determined. The initial mass of the p-aminophenol used was
3.24 grams. The mass of the crude product produced was 3.92 grams and that was recrystallized
to produce 3.44 grams of the pure product. Samples of the crude and pure product were used to
measure melting temperature ranges for both products. It was predicted that the pure product
would have a higher melting temperature range due to the product having stronger bonds than
the less pure, crude product. These predictions were correct, as the melting temperature range of
the crude product was 163oC to 165oC and the pure product was 163oC to 168oC. Looking at the
experimental yield, 3.44 grams of pure product was obtained. However, the calculated theoretical
yield for the acetaminophen was 4.49 grams. This resulted in a percent error of 23.4%. This was
an extremely reliable experiment as there were very few reactions, and more steps involving
changes of state and isolating the precipitate. However, the experimental yield was lower than
the theoretical yield. This could have been due to the dissolving step. When the acetaminophen
was precipitated out of solution and separated out of the solution using vacuum filtration, some
of the acetaminophen could have still been dissolved in solution and didn’t precipitate out. This
could be the main reason for the experimental yield being lower than the theoretical yield.
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References
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