Title | Spectrophotometric Analysis of Aspirin |
---|---|
Course | General Chemistry Lab A |
Institution | Loyola University Chicago |
Pages | 6 |
File Size | 270.7 KB |
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Lab report for Chem 111...
Spectrophotometric Analysis of Aspirin Megan Alagna and Veronica, November 19, 2019, Chemistry 111-008, Dr. Lin, TA Nick
Introduction Aspirin is one of the most commonly used pain relievers because of its effectiveness and its active ingredient, acetylsalicylic acid. This over-the-counter drug is used to treat inflammation, fever, headaches, muscle aches, and various other symptoms. Aspirin, a member of the non-steroid antiinflammatory drug family (NSAIDs), deactivates the enzyme cyclooxygenase (COX), which is responsible for the synthesis of prostanoids, including prostaglandins (PGs) that cause swelling, fever, pain, and inflammation.1 It quickly became popular throughout the world in the 1900s, becoming the most popular painkiller in the Guinness Book of World Records in 1950 and brought on the first spaceship to the Moon in 1969. Earlier versions of aspirin include the use of willow leaves, myrtle leaves, and other extracts of
plants.2 Today, it comes in the form of tablets, liquids, and powders. Some side effects of aspirin may include gastrointestinal bleeding and digestive complications if taken in large quantities, so it is best to take the recommended dosage of aspirin that primary care providers and pharmaceutical companies suggest.3 This experiment will determine the amount of acetylsalicylic acid (ASA) in a standard aspirin tablet using spectrophotometric analysis of a solution containing acetylsalicylic acid and iron (III) ion, which forms a purple solution that can determine the quantification of aspirin through the color intensity using a colorimeter and LabQuest2. Using Beer-Lambert’s Law, which is an equation that states that absorption of light is independent of its intensity and that the amount of light absorbed is directly related to the number of
molecules of absorbing substance through
Values were adjusted for the stock solution
which the light passes, absorbance can be
concentration (1.99 x 103 mg/L) according
determined.4
to the amount measured, which was .498
𝐴=𝜖𝑏𝐶
(Eq. 1)
grams. The wavelength for this experiment
The addition of the iron (III) creates the
was measured at 536.5 nanometers (nm)
complex found in Equation 2.4
within the 500-550 nm range in order to find absorbance. Results
(Eq. 2) The linear equation provided by the
Table 1 Mass/Concentration of ASA and Aspirin Tablet
LabQuest2 using data from stock solutions
Acetylsalicylic Aspirin
of salicylate dianion, formed by aspirin
Acid
Tablet
39.401 g
31.408 g
39.899 g
31.787 g
0.498 g
0.379 g
reacting with sodium hydroxide, will
Mass of flask
provide the necessary data in order to
(g)
calculate the actual amount of acetylsalicylic
Mass of flask
acid in a standard aspirin tablet. This
and
complex is shown in Equation 3.4
compound (g) Mass of compound (g)
(Eq. 3) Experimental
Concentration
1.99 x 103
of ASA in
mg/L
stock solution All of the steps of the experiment were followed according to the lab manual.4
(mg/L)
After taking the masses of both the ASA and
The linear equation (y=mx+b) for the
aspirin solutions, the concentrations of five
concentration and absorbance of ASA was
amounts of ASA were taken as directed in
used as a guide to determine the
the Lab Manual.4 The concentrations and
concentration and absorbance of the
absorbances of each amount of stock
unknown solution of aspirin.
solution were used to determine the linear equation in Figure 1. Table 2 Concentration and Absorbance of Solutions
𝑦 = 0.0059857𝑥 − 0.027239
(Eq. 4)
The interpolation value of aspirin was used to find a concentration of 53.8 mg/L and the
Solution
Conc. (mg/L) Absorbance
A
39.8 mg/L
0.210
B
59.7 mg/L
0.322
C
79.6 mg/L
0.466
absorbance was plugged into the linear
D
99.5 mg/L
0.564
equation, the x-value was 53.8 mg/L, which
E
119.4 mg/L
0.685
Unknown
53.8 mg/L
0.295
absorbance was found at 0.295 when inserted into the spectrovis. When the
is the same as the interpolation value. The
(interpolation
concentration of the unknown aspirin
value)
solution was then used to determine the
Figure 1 Concentration and Absorbance of ASA in a linear equation
amount of ASA in grams using a standard value (325 mg) provided by the lab manual.4 𝑚𝑔 10−3 𝐿 (50.0 ) = 2.69 𝑚𝑔 (53.8 ) 𝑚𝐿) ( 1𝑚𝐿 𝐿 (Eq. 5) 2.69 𝑚𝑔 × 250.0 𝑚𝐿 = 336.25 𝑚𝑔 2.00 𝑚𝐿 = .336 𝑔
(Eq. 6)
By dividing the measured number of grams
536.5 nm was found in the green section of
in the aspirin tablet by the amount found in
the color spectrum, which is directly
the unknown concentration, a percentage of
opposite of the color purple on the color
88.7% ASA was determined.
wheel.
. 336 𝑔 × 100% = 88.7% . 379 𝑔 (Eq. 7)
Percent error was 3.38% using 325 mg as the theoretical and 336 mg as the experimental. Figure 2 The color wheel 336.25 𝑚𝑔 − 325 𝑚𝑔 × 100% = 3.38%. 325 𝑚𝑔 (Eq. 8)
The class average for the mass of aspirin in the tablet was 365 mg, and the average
Discussion percent of ASA in the tablet was 96.9%. The The amount of acetylsalicylic acid in the average percent error was 10.30%, which is given aspirin tablet, which had a mass of higher than the percent error of this 379 mg, was 336 mg as shown in Equation experiment (3.38%). Possible errors could 6. This meant that 88.7% of the aspirin have occurred during the selection of the tablet was acetylsalicylic acid. The wavelength (536.5 nm) or during usage of acidification of the iron (III) ion to change the cuvette, where it could have become the color of the concentrations to purple was foggy. The data might have been more used with the knowledge of the differing accurate if a different wavelength was wavelengths of the color wheel. A value of selected. By using spectrophotometry to
determine the amount of an unknown
found and what was shown in the resulting
substance in a compound such as ASA in
measurements.
aspirin, other substance amounts can also be determined using this method and can help
References
pharmaceutical companies measure the
(1) Vane, J.R.; Botting, R.M.; The
correct amount of active ingredient to add to
Mechanism of Action of Aspirin;
a given medicine.
Thrombosis Research; Volume 110, Issues 5-6; June 2003, pp. 255-258.
Conclusion
https://www.sciencedirect.com/science/articl
6 solutions were measured using a
e/pii/S0049384803003797
spectrophotometer to determine the amount
(2) Jack, D.B.; One Hundred Years of
of acetylsalicylic acid, the active ingredient
Aspirin; The Lancet; Volume 350, August
in aspirin. Solutions A-E were created using
9, 1997, pp. 437-439.
only ASA while the sixth unknown solution
https://www.thelancet.com/journals/lancet/ar
was created using an aspirin tablet. The
ticle/PIIS0140-6736(97)07087-6/fulltext
concentrations of solutions A-E were used to
(3) Huang, E.S.; Strate, L.L.; Ho, W.W.;
then determine an interpolation value for the
Lee, S.S.; Chan, A.T. Long Term Use of
unknown aspirin solution, which was then
Aspirin and the Risk of Gastrointestinal
used to calculate the percent of ASA
Bleeding; The American Journal of
(88.7%) and amount in milligrams of ASA
Medicine, May 2011,
(336 mg). The given amount on the label of
https://www.ncbi.nlm.nih.gov/pmc/articles/P
the aspirin was 325 mg, which shows an
MC3086018/.
inconsistent amount between what was
(4) Spectrophotometric Analysis of Aspirin; Chem 111 Laboratory Manual Fall 2019, pp. 43-48...