Experiment 7.B Name CareL Emcassead Section -D0X Data and Results: Preparation o

Question

Experiment 7.B Name CareL Emcassead Section -D0X Data and Results: Preparation of Aspirin S oeMass of salicylic acid used Volume of acetic anhydride used mL. Mass of acetic anhydride used (density 1.08 g/mL) Mass of aspirin obtained Theoretical yield of aspirin Percentage yield of aspirin 2. 8 Melting point of aspirin oC 12-28 Absorbance of aspirin solution Percentage of salicylic acid impurity Solubility properties of aspirin Toluene Ethyl alcohol Hexane Acetone Ethyl acetate5 Water SS S soluble I insoluble ss-slightly solubl Underline those characteristics listed which would be likely to be present in a good solven for aspirin. organic aliphatic polar hydrogen bonding. inorganic aromatic nonpolar nonhydrogen bonding

Explanation / Answer

3: mass of acetic anhydride used = Volume x density = 5.00 mL x 1.08 g/mL = 5.4 g

5: Moles of salicyclic acid taken = mass/molar mass = 2.00 g / 138.1 g/mol = 0.0145 mol

moles of acetic anhydride taken = mass / molar mass = 5.4 g / 102.09 g/mol = 0.0529 mol

The balanced chemical reaction for the formation of Aspirin is

Salicyclic acid + Acetic anhydride ------- > Aspirin + Acetic acid.

Hence 1 mol of Salicyclic acid reacts with 1 mol of Acetic anhydride to form 1 mol of Aspirin.

Hence 0.0145 mol salicyclic acid will react with 0.0145 mol acetic anhydride to form 0.0145 mol Aspirin

Hence moles of aspirin formed = 0.0145 mol

molar mass of aspirin = 180.15 g/mol

Hence theoritical mass of aspirin formed = 0.0145 mol x 180.15 g/mol = 2.61 g

Hence theoritical yield of aspirin = 2.61 g

6: Percentage yield of Aspirin = (actual yield / theoritical yield) x 100 = (2.8 g / 2.61 g) x 100 = 107 %

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