Question

1.0.980 g of acetylsalicylic acid was obtained from 1.00 g of salicylic acid by reaction with excess acetic anhydride. Calculate the percent yield of acetylsalicylic acid. 2. Two esters with the empirical formula C3H602 may be prepared. Write structural formulas for these esters and name them 3. How would you prepare the two esters in question 2? Draw a reaction for each. 1. Explain why you would or would not expect to observe a color change if FeClj were to the following (a) Pure aspirin он C-OCH, Methyl salicylate 2. Write the structure of the products that you would expect from the following reactions сон CH,CH OH (b) CH,CH OH+ acetic anhydride

Answer 1

1)Mass of salicyllic acid( C,HO) 1.00g Atomic mass of C,H60,-1 381 2 g/m ol No of moles of C,H,O, present 1.00 CHO 6138.12 0.00724 mol C,H,O3 Equation: 4HO3CHCoHO C2H402 Theoretical yiled of C9H8O4 produced = 0.00724 mo LgH襾 1 mol GHO 180.157 g CoHeo - 1.30 g Theoretical yield of aspirin GH804 = 1.30 g Actual yiel dof aspirin CoHgO4 0.980 g Percent yield- _Actual yield Theoretical yiel x100 0.980 8xỉ 00 1.30 g = 75.1% =75%