I can’t figure out question 7 and the last EXPLANATION.. I don’t know if I am doing it right. DAY 2. Percent Acetylsalicylic Acid in the Aspirin SampleCalculation for the mass of aspirin for the titrimetric analysisB.Trial 1Trial 20.3649 Q.36301mollL355ml y5.aml163m17.8178XD3 1.94x1031. Mass of the aspirin sample (g)2. Molar concentration of theNaOH solution (mol/L)3. Buret reading, final (ml)4. Buret reading, initial (ml)5. Volume of NaOH used (ml)6. Amount of NaOH added (mol)7. Amount of acetylsalicylic acidIn the aspirin sample (mol)8. Mass of acetylsalicylic acid (g)9. Percent acetylsalicylic acid inthe aspirin sample (%)ab28%.079ga18%.10. Average percent acetylsalicylicacid in the aspirin sample (%)Explanations: If your yield is low or purity is not 100% provide an explanation below to accountfor the discrepancy.

Given: The molarity of the NaOH solution is 0.1 mol/L. The mass of the aspirin sample taken in trial…

B. DAY 2. Percent Acetylsalicylic Acid in the Aspirin Sample Calculation for the mass of aspirin for the titrimetric analysis Trial 1 Trial 2 0.3643 0.363 g 1. Mass of the aspirin sample (g) 2. Molar concentration of the NaOH solution (mol/L) 355ml y5.am! 3. Buret reading, final (ml) 4. Buret reading, initial (ml) 17.8 190Amlm 5. Volume of NaOH used (ml) 1.78XD3 1.94X103 6. Amount of NaOH added (mol) 7. Amount of acetylsalicylic acid In the aspirin sample (mol) 0సంధి భా a0.28%. 8. Mass of acetylsalicylic acid (g) 9. Percent acetylsalicylic acid in the aspirin sample (%) 10. Average percent acetylsalicylic acid in the aspirin sample (%) Explanations: If your yield is low or purity is not 100% provide an explanation below to account for the discrepancy.