Experiment: analysis aspirin using acid_base titration Purpose: To determine the amount of active ingredient in an aspirin tablet Theory: Aspirin ( ₃ ₆₄ ) contains a carboxyl (− ) functional group. It can react with sodium hydroxide, hence the amount of aspirin in aspirin tablets can be determined by performing a titration using sodium hydroxide solution. Materials: 3 aspirin tablets 10 mL measuring cylinder 30 mL methylated spirits Burette, retort stand and burette clamp 100 mL 0.1 M standard sodium hydroxide solution White tile 20 mL 0.1 M hydrochloric acid Stirring rod Phenolphthalein indicator Deionized water 100 mL conical flasks (3) Safety: Methylated spirits is highly flammable, keep it away from flames Sodium hydroxide solution is an irritant to skin and eyes Wear safety glasses, gloves and a laboratory coat for eye and skin protection Procedure: 1. Record the brand of aspirin tablets used in this experiment; and the mass of each tablet as specified by the manufacturer. 2. Transfer an aspirin tablet to a clean 100 mL conical flask; add about 10 mL methylated spirits. 3. Crush any large lumps of aspirin tablet with a stirring rod, swirl the conical flask until almost all the tablet dissolves. Add 20 mL deionized water to the flask. 4. Record the concentration of a standard solution of sodium hydroxide. Rinse and fill a burette with this solution. Write the initial burette reading to two decimal places. 5. Add 3 drops of phenolphthalein indicator to the aspirin solution and titrate with sodium hydroxide solution until the first permanent pink appears in the flask. Record the final burette reading. 6. Repeat steps 2 to 5 twice. 7. When cleaning up, thoroughly rinse the burette with water, followed by a small volume of dilute hydrochloric acid, and more water. Question 1: if the traces of aspirin is not washed off the stirring rod back into the conical flask, what might be the effect on the average mass of aspirin ?. Explain. Question 2: What are some of the possible sources of error in this experiment?
Experiment: analysis aspirin using acid_base titration Purpose: To determine the amount of active ingredient in an aspirin tablet Theory: Aspirin ( ₃ ₆₄ ) contains a carboxyl (− ) functional group. It can react with sodium hydroxide, hence the amount of aspirin in aspirin tablets can be determined by performing a titration using sodium hydroxide solution. Materials: 3 aspirin tablets 10 mL measuring cylinder 30 mL methylated spirits Burette, retort stand and burette clamp 100 mL 0.1 M standard sodium hydroxide solution White tile 20 mL 0.1 M hydrochloric acid Stirring rod Phenolphthalein indicator Deionized water 100 mL conical flasks (3) Safety: Methylated spirits is highly flammable, keep it away from flames Sodium hydroxide solution is an irritant to skin and eyes Wear safety glasses, gloves and a laboratory coat for eye and skin protection Procedure: 1. Record the brand of aspirin tablets used in this experiment; and the mass of each tablet as specified by the manufacturer. 2. Transfer an aspirin tablet to a clean 100 mL conical flask; add about 10 mL methylated spirits. 3. Crush any large lumps of aspirin tablet with a stirring rod, swirl the conical flask until almost all the tablet dissolves. Add 20 mL deionized water to the flask. 4. Record the concentration of a standard solution of sodium hydroxide. Rinse and fill a burette with this solution. Write the initial burette reading to two decimal places. 5. Add 3 drops of phenolphthalein indicator to the aspirin solution and titrate with sodium hydroxide solution until the first permanent pink appears in the flask. Record the final burette reading. 6. Repeat steps 2 to 5 twice. 7. When cleaning up, thoroughly rinse the burette with water, followed by a small volume of dilute hydrochloric acid, and more water. Question 1: if the traces of aspirin is not washed off the stirring rod back into the conical flask, what might be the effect on the average mass of aspirin ?. Explain. Question 2: What are some of the possible sources of error in this experiment?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Experiment: analysis aspirin using acid_base titration
Purpose: To determine the amount of active ingredient in an aspirin tablet
Theory: Aspirin ( ₃ ₆₄ ) contains a carboxyl (− ) functional group. It can react with
sodium hydroxide, hence the amount of aspirin in aspirin tablets can be determined by performing a titration
using sodium hydroxide solution.
Materials:
3 aspirin tablets 10 mL measuring cylinder
30 mL methylated spirits Burette, retort stand and burette clamp
100 mL 0.1 M standard sodium hydroxide solution White tile
20 mL 0.1 M hydrochloric acid Stirring rod
Phenolphthalein indicator Deionized water
100 mL conical flasks (3)
Safety:
Methylated spirits is highly flammable, keep it away from flames
Sodium hydroxide solution is an irritant to skin and eyes
Wear safety glasses, gloves and a laboratory coat for eye and skin protection
Procedure:
1. Record the brand of aspirin tablets used in this experiment; and the mass of each tablet as specified by
the manufacturer.
2. Transfer an aspirin tablet to a clean 100 mL conical flask; add about 10 mL methylated spirits.
3. Crush any large lumps of aspirin tablet with a stirring rod, swirl the conical flask until almost all the tablet
dissolves. Add 20 mL deionized water to the flask.
4. Record the concentration of a standard solution of sodium hydroxide. Rinse and fill a burette with this
solution. Write the initial burette reading to two decimal places.
5. Add 3 drops of phenolphthalein indicator to the aspirin solution and titrate with sodium hydroxide
solution until the first permanent pink appears in the flask. Record the final burette reading.
6. Repeat steps 2 to 5 twice.
7. When cleaning up, thoroughly rinse the burette with water, followed by a small volume of dilute hydrochloric acid, and more water.
Question 1: if the traces of aspirin is not washed off the stirring rod back into the conical flask, what might be the effect on the average mass of aspirin ?. Explain.
Question 2: What are some of the possible sources of error in this experiment?.
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