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D. Using Your Spectrophotometer SpectroVis Plus Settings Mode (%T, Kinetic, Abs, etc.?) _________________________ Wavelength (nm) _________________________ 10nm band or Individual Wavelength _________________________ E. Determination of λ max 1. The data table showing the absorbance of your approximately 4.4 × 10-4 mol ⋅ L-1 solution at all the wavelengths (nm) will be many pages long. Do not print it all off. Instead just show the raw data for the part of the scan that shows where the λ max occurs plus and minus 15 nm. 2. Plot a graph of absorbance (y axis) vs. wavelength (x axis). Identify the wavelength at which the absorbance is at a maximum. F. Construction of a Calibration Curve 1. Prepare a table that shows the absorbance for each of your six dilute solutions and the blank (0.02 M FeCl3). 2. Plot a graph of Absorbance (y axis) vs. concentration (x axis). G. Determination of the Concentration of the Solution Prepared from Commercial Aspirin® or generic brand 1. The absorbance of diluted solution prepared from ASA tablet was _______ (absorbance units). 2. From the graph plotted in F, such an absorbance corresponds to a concentration of ______________ M ASA. H. Determination of the Percentage of Acetylsalicylic Acid in an Aspirin® or generic brand Tablet 1. From G, the concentration of tetraaquasalicylatoiron(III) in the dilute solution was ______________. 2. The concentration of the dianion of salicylic acid in the 100 mL sodium hydroxide stock solution was ______________. 3. The number of moles of the dianion of salicylic acid in the 100mL sodium hydroxide stock solution was ______________. 4. The number of moles of acetylsalicylic acid initially present and therefore also in the Aspirin® tablet was ______________. 104 5. The mass of acetylsalicylic acid in the Aspirin® tablet was __________. 6. The percentage of acetylsalicylic acid in the Aspirin® tablet was _____. WARNING: As with all the experiments in this course, your grade for this experiment will depend primarily on the accuracy and precision of your results. Do not proceed to the next experiment until you are satisfied that you have completed this experiment to the best of your ability

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Laboratory Report Experiment A3
Title: Acid-Base Titrations

Purpose: The purpose of this lab is to acquire and be acclimatized through the theories of acid-base titrations. It comprises the mole concept and stoichiometry involved in the reaction. To understand the process of dilution and the net molecular as well as ionic equation involved in the acid-base titration. It also helps in proper operation and handing of burette. Demonstration of neutralization process and calculations involved therein. Also it is involved prediction the concentration of unknown aspirin concentration.
The chemical equation presented below for the neutralization:
                                     H+ + OH- → H2O + heat
      Acid      Base       Water
Aspirin is a non-steroidal anti-inflammatory drug (NSAIDs) which is used as a painkiller and originally discovered from salicylic acid. It’s an acid, therefore, it can be analyzed by acid-base titration using standardized sodium hydroxide solution. But there are some practical problems (due to weak acid nature of aspirin and ester is being hydrolyzed) in direct titration, therefore “back titration” is preferred, which involved reaction of NaOH (base) in excess and later the remaining base is analyzed by hydrochloric acid....

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