To calculate the theoretical yield of aspirin, we need to use the stoichiometry of the balanced chemical equation for the synthesis of aspirin from salicylic acid and acetic anhydride. The balanced equation is:C7H6O3 salicylic acid + C4H6O3 acetic anhydride C9H8O4 aspirin + C2H4O2 acetic acid From the balanced equation, we can see that 1 mole of salicylic acid reacts with 1 mole of acetic anhydride to produce 1 mole of aspirin.First, we need to find the moles of salicylic acid and acetic anhydride.Molar mass of salicylic acid C7H6O3 = 7 12.01 + 6 1.01 + 3 16.00 = 138.12 g/molMoles of salicylic acid = mass / molar mass = 5 g / 138.12 g/mol = 0.0362 molNext, we need to find the moles of acetic anhydride. The density of acetic anhydride is approximately 1.08 g/mL.Mass of acetic anhydride = volume density = 10 mL 1.08 g/mL = 10.8 gMolar mass of acetic anhydride C4H6O3 = 4 12.01 + 6 1.01 + 3 16.00 = 102.09 g/molMoles of acetic anhydride = mass / molar mass = 10.8 g / 102.09 g/mol = 0.1058 molSince the stoichiometry of the reaction is 1:1, the limiting reagent is salicylic acid 0.0362 mol because it is present in a smaller amount.Now, we can calculate the theoretical yield of aspirin.Molar mass of aspirin C9H8O4 = 9 12.01 + 8 1.01 + 4 16.00 = 180.16 g/molTheoretical yield of aspirin = moles of limiting reagent molar mass of aspirin = 0.0362 mol 180.16 g/mol = 6.52 gTherefore, the theoretical yield of aspirin that can be obtained from the synthesis of 5 grams of salicylic acid using 10 mL of acetic anhydride, assuming a 100% yield and purity, is 6.52 grams.