Data Set Exp.5Use the following data to determine the masspercent of the active ingredient in Aspirina) Preparation of solutions:volume of salicylic acidvolume ofFECL3 solutionSA11ml9mlSA23.5ml6.5mlSA36.5ml3.5mlSA41ml9mlThe concentration of salicylic acid= 0.000725Mb) Preparation of "STOCK ASAUNKNOWN"The mass of aspirin= 0.135 gThe volume of stock solution of aspirin= 100mlThe dilution factor for the stock solution= 50/2Molar mass of SAS = 180.157 g/molec) Measurements of Absorbance:SolutionAbsorbanceSA10.154SA20.524SA30.789SA40.989The unknown sample0.259 A) Standard solution and Beer's law calibration curve1-Fill in the following table :Concentration For S.1 M¸ x V = M, x V 0.000725 x 1.0ml = M, x 10.0mlSolutionAbsorbanceConcentrationS. 1S.2S.3S.4ASA of unknown6666666662- Plot a graph of Absorbance vs. conc mol / LabsorbanceAbsorbance vs. Concentration1.61.41.210.8OY-Values0.60.40.26.10conc 104 mol/ LB) Analvsis of unknown aspirin tablet1. Mass of aspirin tablet =g2. Concentration of ASA unknown from calibration curvemol / L3.. Conc of Stock ASA unknown = 50 mL / 1.5 mL (D.F) x Conc of ASA unknownmol / L4. Moles of ASA in 100 mL solution = Conc of Stock ASA unknown x 0.1 L=moles5.Mass of ASA = moles ASA x Molar Mass ASA (180 g/ mol) =6. % of ASA in aspirinMass of ASA / Mass of aspirin tablet x100 =%3D

Calibration curve It is the standard curve used to determine the concentration of unknown sample…

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