Data Set Exp.5 Use the following data to determine the mass percent of the active ingredient in Aspirin a) Preparation of solutions: volume of salicylic acid volume of FECL3 solution SA1 1ml 9ml SA2 3.5ml 6.5ml SA3 6.5ml 3.5ml SA4 1ml 9ml The concentration of salicylic acid= 0.000725M b) Preparation of “STOCK ASA UNKNOWN" The mass of aspirin= 0.135 g The volume of stock solution of aspirin= 100ml The dilution factor for the stock solution= 50/2 Molar mass of SAS = 180.157 g/mole c) Measurements of Absorbance: Solution Absorbance SA1 0.154 SA2 0.524 SA3 0.789 SA4 0.989 The unknown sample 0.259

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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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Data Set Exp.5
Use the following data to determine the mass
percent of the active ingredient in Aspirin
a) Preparation of solutions:
volume of salicylic acid
volume of
FECL3 solution
SA1
1ml
9ml
SA2
3.5ml
6.5ml
SA3
6.5ml
3.5ml
SA4
1ml
9ml
The concentration of salicylic acid= 0.000725M
b) Preparation of "STOCK ASA
UNKNOWN"
The mass of aspirin= 0.135 g
The volume of stock solution of aspirin= 100ml
The dilution factor for the stock solution= 50/2
Molar mass of SAS = 180.157 g/mole
c) Measurements of Absorbance:
Solution
Absorbance
SA1
0.154
SA2
0.524
SA3
0.789
SA4
0.989
The unknown sample
0.259
Transcribed Image Text:Data Set Exp.5 Use the following data to determine the mass percent of the active ingredient in Aspirin a) Preparation of solutions: volume of salicylic acid volume of FECL3 solution SA1 1ml 9ml SA2 3.5ml 6.5ml SA3 6.5ml 3.5ml SA4 1ml 9ml The concentration of salicylic acid= 0.000725M b) Preparation of "STOCK ASA UNKNOWN" The mass of aspirin= 0.135 g The volume of stock solution of aspirin= 100ml The dilution factor for the stock solution= 50/2 Molar mass of SAS = 180.157 g/mole c) Measurements of Absorbance: Solution Absorbance SA1 0.154 SA2 0.524 SA3 0.789 SA4 0.989 The unknown sample 0.259
A) Standard solution and Beer's law calibration curve
1-Fill in the following table :
Concentration For S.1 M¸ x V = M, x V 0.000725 x 1.0ml = M, x 10.0ml
Solution
Absorbance
Concentration
S. 1
S.2
S.3
S.4
ASA of unknown
666666666
2- Plot a graph of Absorbance vs. conc mol / L
absorbance
Absorbance vs. Concentration
1.6
1.4
1.2
1
0.8
OY-Values
0.6
0.4
0.2
6.
10
conc 104 mol/ L
B) Analvsis of unknown aspirin tablet
1. Mass of aspirin tablet =
g
2. Concentration of ASA unknown from calibration curve
mol / L
3.. Conc of Stock ASA unknown = 50 mL / 1.5 mL (D.F) x Conc of ASA unknown
mol / L
4. Moles of ASA in 100 mL solution = Conc of Stock ASA unknown x 0.1 L=
moles
5.Mass of ASA = moles ASA x Molar Mass ASA (180 g/ mol) =
6. % of ASA in aspirin
Mass of ASA / Mass of aspirin tablet x100 =
%3D
Transcribed Image Text:A) Standard solution and Beer's law calibration curve 1-Fill in the following table : Concentration For S.1 M¸ x V = M, x V 0.000725 x 1.0ml = M, x 10.0ml Solution Absorbance Concentration S. 1 S.2 S.3 S.4 ASA of unknown 666666666 2- Plot a graph of Absorbance vs. conc mol / L absorbance Absorbance vs. Concentration 1.6 1.4 1.2 1 0.8 OY-Values 0.6 0.4 0.2 6. 10 conc 104 mol/ L B) Analvsis of unknown aspirin tablet 1. Mass of aspirin tablet = g 2. Concentration of ASA unknown from calibration curve mol / L 3.. Conc of Stock ASA unknown = 50 mL / 1.5 mL (D.F) x Conc of ASA unknown mol / L 4. Moles of ASA in 100 mL solution = Conc of Stock ASA unknown x 0.1 L= moles 5.Mass of ASA = moles ASA x Molar Mass ASA (180 g/ mol) = 6. % of ASA in aspirin Mass of ASA / Mass of aspirin tablet x100 = %3D
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