In an organic chemistry lab a student prepared aspirin by reacting salicylic acid and acetic anhydride, while using sulfuric acid as a catalyst. The table below shows data from this experiment. Mass of salicylic acid 4.0g Volme of acetic anhydride 6.0 ml. Volume of sulfuric acid 0.5 ml. Percentage yield 92 % () Cakulate the actual mass of aspirin obtained from this experiment. (i) State two methods that can be used to confirm the purity of the product obtained.
In an organic chemistry lab a student prepared aspirin by reacting salicylic acid and acetic anhydride, while using sulfuric acid as a catalyst. The table below shows data from this experiment. Mass of salicylic acid 4.0g Volme of acetic anhydride 6.0 ml. Volume of sulfuric acid 0.5 ml. Percentage yield 92 % () Cakulate the actual mass of aspirin obtained from this experiment. (i) State two methods that can be used to confirm the purity of the product obtained.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![1.
(a)
In an organic chemistry lab a student prepared aspirin by reacting salicylic acid and acetic
anhydride, while using sulfuric acid as a catalyst. The table below shows data from this
еxperiment.
Mass of salicylic acid
4.0 g
Volume of acetic anhydride 6.0 mL
Volume of sulfuric acid
0.5 ml.
Percentage yield
92 %
(i) Cakulate the actual mass of aspirin obtained from this experiment.
(i) State two methods that can be used to confirm the purity of the product obtained.
(b)
An experiment was carried out as follows: 1.5766 g of an ammonium salt was placed in a beaker
and 60 mL of 1.182 M sodium hydroxide was added. The resulting mixture was heated for about
an hour and then left to cool to room temperature. The reaction mixture was then titrated with
sulfuric acid and required 18.35 ml. of the acid for complete neutralization. Given that the
percentage by mass of ammonium in the salt was 37.5 %, calculate the molarity of the sulfurie
acid used in the titration.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F591cafb9-b3e1-475e-ae1d-e861d0e5b3ea%2F4453e561-09b9-4e43-b84f-a36e38094645%2F6cb419a_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1.
(a)
In an organic chemistry lab a student prepared aspirin by reacting salicylic acid and acetic
anhydride, while using sulfuric acid as a catalyst. The table below shows data from this
еxperiment.
Mass of salicylic acid
4.0 g
Volume of acetic anhydride 6.0 mL
Volume of sulfuric acid
0.5 ml.
Percentage yield
92 %
(i) Cakulate the actual mass of aspirin obtained from this experiment.
(i) State two methods that can be used to confirm the purity of the product obtained.
(b)
An experiment was carried out as follows: 1.5766 g of an ammonium salt was placed in a beaker
and 60 mL of 1.182 M sodium hydroxide was added. The resulting mixture was heated for about
an hour and then left to cool to room temperature. The reaction mixture was then titrated with
sulfuric acid and required 18.35 ml. of the acid for complete neutralization. Given that the
percentage by mass of ammonium in the salt was 37.5 %, calculate the molarity of the sulfurie
acid used in the titration.
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