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Preparation of Aspirin sample

Tare a small beaker or weighing dish. Add an aspirin tablet to the beaker and record the mass to the nearest 0.001g.
Add 5 ml of 1M NaOH to the flask and wash down the inside of the flask with 20-30mls of distilled water. Using a hot plate, boil this solution for 10-15min. Don’t allow all of the water to boil off. Avoid splattering and loss of contents.: NaOH is harmful to the skin and eyes. Rinse the inside walls of the flask with small portions (3-5ml) of distilled water several times to ensure quantitative conversion of the acetylsalicylic acid to salicylate ion.
Allow the solution to cool to room temperature. While the solution cools, obtain a clean 100 ml volumetric flask.
Quantitatively transfer the solution of sodium salicylate to the clean 100 ml volumetric flask and dilute with distilled water to the mark. Thoroughly mix this solution by inverting the volumetric flask several times. Label as “MY ASPIRIN STOCK SOLUTION.”
Transfer 200 ml into a 10ml volumetric flask and dilute to the mark with 0.02M FeCl3 solution. Thoroughly mix this solution by inverting the volumetric flask several times. Label as “MY ASPIRIN diluted”

Preparation of Standards

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Tare a second small beaker or weighing dish. Measure out approximately 0.160 of pure salicylic acid to the flask and record the mass to the nearest 0.001g. Note: it is not important that you get exactly 0.160 g. It is important that you record the exact mass of salicylic acid that you measured out.
Add 5 ml of 1M NaOH to the flask and wash down the inside of the beaker with 20-30mls of distilled water. Using a hot plate, boil this solution for 10-15min. DO NOT allow all of the water to boil off. Avoid splattering and loss of contents. CAUTION: NaOH is harmful to the skin and eyes. Rinse the inside walls of the flask with small portions (3-5ml) of distilled water several times to ensure quantitative hydrolysis of the acetylsalicylic acid.
Allow the solution to cool to room temperature. While the solution cools, obtain a 100 ml volumetric flask and clean several times with distilled water.
Quantitatively transfer the solution of sodium salicylate to the clean 100 ml volumetric flask and dilute with distilled water to the mark. Thoroughly mix this solution by inverting the volumetric flask several times. Label as “STANDARD STOCK SOLUTION.”
Prepare five 10ml volumetric flasks (A-E). In each one, put the volume ( in ml) of stock solution indicated in the table below and add 0.02M FeCl3 solution to the mark. Thoroughly mix each standard solution by inverting a number of times.

Solution ml of Stock
A 100
B 200
C 300
D 400
E 500

Measure the absorbance of each solution (wavelength = 530nm). To blank the UV-Vis Spec, add 0.02 M FeCl3 to the cuvette and press blank. Starting with the standards read the absorbance of each and record. Lastly, get the absorbance of synthesized aspirin.
Rinse all of the glassware with distilled water. All materials can be washed down the sink with plenty of water to neutralize the acids and bases.

Data:

Aspirin tablet: 0.421 g

Salicylic Acid standard mass: 0.159 g

Absorbances:
Type of solution/ Absorbance Reading
Standard A 0.137

Standard B 0.306
Standard C 0.518
Standard D 0.699
Standard E 0.823
My Aspirin diluted 0.515

Calculations:
Please show your work for full credit on these calculations.

Calculate the number of moles of pure salicylic acid used in the “STANDARD STOCK SOLUTION”

2.Calculate the molarity of the “STANDARD STOCK SOLUTION”
3.Calculate the molarity of each of the standard solutions (A – E)

4.Plot the concentration of each standard solution (A-E) vs. Absorbance (Beer’s Law plot).
5.Use the absorbance of your ‘MY ASPIRIN diluted’ solution and your Beer’s Law plot to determine the concentration of aspirin in your diluted “MY ASPIRIN” solution.
6.Use the concentration of your diluted “MY ASPIRIN” solution to calculate the molarity, moles, and mass of aspirin in the tablet of aspirin.
7.The common advertised mass of active ingredient in an aspirin tablet is 325 mg. Using this as your accepted value, calculate the percent error of your measurements:

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