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10 Nov 2019

One tablet of Brand Y aspirin was dissolved in 10 mL of 1.0 M NaOH , boiled, and then diluted to a final volume of 100 mL with deionized water. A 2.5 mL aliquot of this concentrated aspirin solution was dieted to a final volume of 100 mL with FeCl3 . A calibration plot of absorbance vs. concentration was obtained , with the slope of the best fit straight line was 1370M-1. The diluted aspirin solution had an absorbance of 0.932. What is the concentration of the dilute aspirin?a. What is the concentration of the aspirin in the dilute aspirin solution?b. What is the concentration of the original solution ?C. How many mg of aspirin are present in one tablet of Brand Y aspirin?

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Irving Heathcote
Irving HeathcoteLv2
6 May 2019

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Related questions

A calibration plot of absorbance vs. concentration was obtained with standard solutions of sodium salicylate, which had a slope of the best-fit straight line as 1750 M–1. The absorbance of a dilute aspirin solution mixed with FeCl3 was 0.88.

(1.) Using Beer's Law, How will the absorbance measured for thesolutions change as the concentration of aspirin in solutionsincrease?

(2.) In an experiment, the Beer’s Law plot resulted in thefollowing relationship between absorbance and concentration of ASA,y = 1061.5x, where y is absorbance and x is the concentration. Ifthe absorbance of a sample solution prepared from an aspirin tabletis 0.402, calculate the concentration of ASA in the solution inM.


(3.) If the above solution was prepared by taking 10 mL of stocksolution and diluting it to 100 mL, what is the concentration ofthe stock solution?


(4.) This stock solution was prepared as follows: An aspirin tabletwas transferred to an Erlenmeyer flask and reacted with NaOH. Theresulting solution was transferred to a 250 mL volumetric flask andthe volume made up to 250 mL. Calculate the mass of aspirin in thetablet based on the concentration of aspirin in the stocksolution.

*The concentration you determined in (3.) is the concentration ofthe solution in molarity. Using this molarity and the volume of thesolution (250 mL), solve for the moles of aspirin in the flask andthe mass of Aspirin in the flask.

A student used standard solutions of aspirin in a FeCl3-KCl-HCl mixture to plot a graph of molarity versus absorbance for diluted aspirin solutions of known concentration. The student determined the slope of the graph to be 4,687 M-1cm-1. Next the student measured out 0.288 grams of a headache medicine tablet and dissolved it in 10.0 ml of NaOH and then added enough water to make a 100 ml solution. Five ml of this solution was then added to another 100 ml flask and diluted to the mark with enough FeCl3-KCl-HCl mixture. The solution was then measured forabsorbency as 0.306

Calculate the molarity of the diluted solution determined from the absorbency and the slope. Then use the molarity of the original solution, its volume and molar mass to calculate the grams of pure acetylsalicylic acid.

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