Determining The Molar Concentration Of Naoh And Hcl Acid
Analytical Chemistry
Experiment 2b: Determination of the ASA Content of Aspirin
Due Date: September 16, 2013
Experiment#: 2b
Title: Determination of the ASA Content of Aspirin
Aim: To determine the Molar Concentration of NaOH and HCl acid used in their Standardization processes and to determine the acetylsalicylic acid (ASA) content in Aspirin.
Materials/Apparatus: materials used are the same as that outlined in the laboratory procedure prepared by the laboratory instructor.
Procedure: The procedure used is the same as that outlined in the laboratory procedure prepared by the laboratory instructor.
Abstract: Aspirin is said to be the oldest and generally most useful drug due to its analgesic and antipyretic properties. Aspirin …show more content…
Of HCl = 1.376 x 10-2L x 1.084×10-1molL-1 =1.492 x 10-3 moles
Number of moles of A.S.A can be found by the difference between the mean number of moles of NaOH added for hydrolysis and the mean number of moles of HCl.
Avg.vol=sample volumes# of samples Avg. vol = (42.83 + 43.40) 2 = 43.12 mL
# of moles of NaOH = Mean vol of NaOH x Molar Conc. Of NaOH = 4.312 x 10-2L ×0.09085molL-1 =3.917 x 10-3 moles
# of mol A.S.A = mean # of moles NaOH - mean # moles HCl = 3.917 x 10-3 moles - 1.492 x 10-3 moles = 2.425 x 10-3 moles Mass of ASA = # of moles x RMM = 2.425 x 10-3 moles x 180.159gmol-1 = 0.437g x 1000 mg 1g = 437mg
Mass% of each sample = mass of A.S.A x 100 mass crushed tablet
mass of sample 1 = 437 mg x 100 503.8 mg = 86.74 %
Mass of sample 2 = 437mg x 100 499.2mg = 87.54%
Mean mass% of A.S.A= 86.74%
Experiment 2b: Determination of the ASA Content of Aspirin
Due Date: September 16, 2013
Experiment#: 2b
Title: Determination of the ASA Content of Aspirin
Aim: To determine the Molar Concentration of NaOH and HCl acid used in their Standardization processes and to determine the acetylsalicylic acid (ASA) content in Aspirin.
Materials/Apparatus: materials used are the same as that outlined in the laboratory procedure prepared by the laboratory instructor.
Procedure: The procedure used is the same as that outlined in the laboratory procedure prepared by the laboratory instructor.
Abstract: Aspirin is said to be the oldest and generally most useful drug due to its analgesic and antipyretic properties. Aspirin …show more content…
Of HCl = 1.376 x 10-2L x 1.084×10-1molL-1 =1.492 x 10-3 moles
Number of moles of A.S.A can be found by the difference between the mean number of moles of NaOH added for hydrolysis and the mean number of moles of HCl.
Avg.vol=sample volumes# of samples Avg. vol = (42.83 + 43.40) 2 = 43.12 mL
# of moles of NaOH = Mean vol of NaOH x Molar Conc. Of NaOH = 4.312 x 10-2L ×0.09085molL-1 =3.917 x 10-3 moles
# of mol A.S.A = mean # of moles NaOH - mean # moles HCl = 3.917 x 10-3 moles - 1.492 x 10-3 moles = 2.425 x 10-3 moles Mass of ASA = # of moles x RMM = 2.425 x 10-3 moles x 180.159gmol-1 = 0.437g x 1000 mg 1g = 437mg
Mass% of each sample = mass of A.S.A x 100 mass crushed tablet
mass of sample 1 = 437 mg x 100 503.8 mg = 86.74 %
Mass of sample 2 = 437mg x 100 499.2mg = 87.54%
Mean mass% of A.S.A= 86.74%