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The purpose of this Titration Analysis of ASA experiment was to use titration analysis techniques to determine the amount of ASA content contained of a standard pain-relief tablet.

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Introduction

Data Collection & Processing: *This Section Includes All Data Processed From the Lab - Data Collection - Tables Of Results: - Table 1: Titration of 10.00 mL of KHP (K4C7HO2COO) With 0.150 mol/L NaOH(aq) Titration of 10.00 mL of KHP (K4C7HO2COO) With 0.150 mol/L NaOH(aq) Trial 1 2 3 4 Final Burette Reading (mL) �0.5ml 13.80 23.50 17.10 38.10 Initial Burette Reading (mL) �0.5ml 4.20 13.80 7.40 28.40 Volume of NaOH(aq) Added (mL) �1.0ml 9.60 9.70 9.70 9.70 Color at Endpoint Light Pink Light Pink Light Pink Light Pink - Table 2: Titration of ASA Tablet With 0.150 mol/L NaOH(aq) Titration of ASA Tablet With 0.150 mol/L NaOH(aq) Trial 1 2 3 Final Burette Reading (mL) �0.5ml 41.00 42.40 15.00 Initial Burette Reading (mL) �0.5ml 27.90 29.40 2.00 Volume of NaOH(aq) Added (mL) �1.0ml 13.10 13.00 13.00 Color at Endpoint Dark Pink Light Pink Light Pink Data Processing: Balanced Chemical Reaction Equation (Used for Molar Ratio and other calculations): NaOH (aq) + KHC8H4O4 (aq)==> NaKC8H4O4 (aq) + H2O (l) Molar Masses of Elements/Solutions Used in this Experiment: Symbol Element Atomic Mass C Carbon 12.01078 H Hydrogen 1.007947 O Oxygen 15.99943 Na Sodium 22.989769282 K Potassium 39.09831 1) ...read more.

Middle

Calculations - Unknown Variable(s): - 325mg of ASA/Tablet - Concentration of KHP(aq): 0.149mol/L KHP(aq) �0.41% - Average NaOH(aq) added to dissolved ASA solution: - Uncertainties Used For Calculations: - Concentration of NaOH(aq): 1.43% - Burette(the uncertainties were not specified on this instrument): 0.10mL Initial reading and final reading to the nearest 0.1mL, since we took 2 measurements to the nearest 0.1mL, the calculation for this uncertainty is 0.05mL2 = 0.10mL *Note: ASA (C9H8O4 (aq))'s state is aqueous because we have crushed the ASA(s) and dissolved it in boiling water) - Final Percent Uncertainty for mass of ASA: 1.43%+1.03%=2.46% ( 361.1916mg =361.19mg (2.46%) - Percent Differential from Accepted Result (325mg): - (361.19 - 325.0)/325 x 100 = 11.13538462% =11.08% - Converted Result: = - Final Result + Uncertainty: 361.1916mg11.08% or 361.19mg End of Data and Processing Section of this lab report, please see next page for the Conclusion and Evaluation of results for this lab. Conclusion & Evaluation: The purpose of this "Titration Analysis of ASA" experiment was to use titration analysis techniques to determine the amount of ASA content contained of a standard pain-relief tablet. According to the product label, the mass of ASA in a standard pain-relief tablet is 325mg, however based on the calculations in my data collection, this result differentiates from my calculation of 361.1916mg of ASA in a standard pain-relief tablet by a factor of approximately +11.08% or +. ...read more.

Conclusion

Aside from the flaws, there are some areas in this experiment that we could have done better. We could have crushed the pills first and then dissolve them in the hot water; I think this method could have resulted a more accurate end result to the experiment if we manage to not lose any crushed powder because the powder would have dissolved much better than the solid pills. The second improvement is that we could have the used less water or more phenolphthalein indicator, since water does not play a part of the reaction process, less water used could have made it for us to identify the change in the color of the solution easier. For the pipette error factor could have been prevent with better equipment, the students in our group found it very difficult to control the pressure of the bulb without losing some solution, I didn't think the pipette with the pressure bulb was the best equipment for accuracy, other pipettes with better methods of solution extraction methods could have been used and improve our final results from differentiating from the accepted value. This experiment was quite challenging because it required many accurate measurements of solutions and excellent observation skills from everyone to record the endpoint of the reaction. ...read more.

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