Hi I appreciate you taking my question. I Want you to explain how to do it. I have no data so please makeup data or variables and show work of how to get points and solving. Thank you! The data table doesn't have to be big since this will serve as a set of examples for me to use.
For the titration of your isolated P8S1 material construct a table that includes the sample of mass titrated, volume and concentration of standardized NaOH for the titration, physical observations/technical problems, and the inferred pKa and molar mass (MM) values. If you ran multiple titrations of your isolate, then expand the table with additional rows, one for each additional trial.
Analyze the above Results Table. For pure aspirin (ASA), pKa = 3.49 and the MM = 180.16 g/mol. While, for pure caffeine, pKa = 14.0 and MM = 194.2 g/mol. Pure HCl has a pKa ≈ -7 in water and MM = 36.46 g/mol. Remember ASA can undergo hydrolysis to salicylic acid (especially at pH ≥ 8) - the pKa and molar mass of pure salicylic acid (SA) are 2.97 and 138.12 g/mol. Incorporating this information clearly state what the titration results indicate about the identity and purity of the isolated material from Project 8, Session 1.
1. Fill a burette with N sodium hydroxide solution.
2. Weigh aspirin into a 250 ml beaker Add 10 cm3 of 95% ethanol, Stir with a glass rod and when the solid has dissolved add 90 cm3 of deionised water. Stir the mixture until it is homogeneous.
3. Place a pH probe in the solution and connect it to a pH meter. Note: The pH probe should have been calibrated using suitable buffer solutions.
4. Add 0.5 cm3 quantities of sodium hydroxide solution from the burette to the beaker, stirring well between additions and recording the pH.
5. Near the end-point the pH begins to rise rapidly.
6. Plot a graph of pH against volume of N sodium hydroxide
7. From the graph, calculate the end-point of the titration.
similarly you can do for caffieine. For HCl no need of ethanol just dilute in water.
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