You add 2.202 g salicylic acid to a 125 mL Erlenmeyer flask. You add 4.0 mL...

You add 2.202 g salicylic acid to a 125 mL Erlenmeyer flask. You add 4.0 mL acetic anhydride and 5 drops of sulfuric acid. After completing the synthesis, filtering, you place the crystals to dry on an evaporating dish that weights 22.067 g. After drying, the crystals and evaporating dish weigh 24.452 g. Calculate the percent yield of aspirin.

Solutions

Expert Solution

Salicylic acid + Acetic anhydride -----> Aspirin + Acetic acid

1 mole 1 mole 1mole 1mole

Actual yield

Empty weight of the dish = 22.067g

After drying empty dish + Crystals = 24.452g

Weight of Crystals = 2.385g

Actual yield = 2.385g

Theoretical yield

weight of salicylic acid = 2.202g

Molar mass of salicylic acid = 138.12g

No of mole of salicylic acid = 2.202/138.12= 0.01594

Volume of acetic anhydride = 4 ml

Density of acetic anhydride = 1.082g/ml

Mass of acetic anhydride = 1.082 ×4 = 4.328g

Molar mass of acetic anhydride =102.09g

No of mole of acetic anhydride = 4.328/102.09= 0.04239

According to stoichiometry salicylic acid is limiting

1 mole of salicylic acid gives 1mole of aspirin

0.01594 mole of salicylic acid give 0.01594 mole of aspirin

Molar mass of aspirin = 180.16g

Mass of aspirin = 0.01594 × 180.16g = 2.872g

Percentage yield

Percentage yield =( Actual yield/Theoretical yield)×100

= (2.385g/2.872g) ×100

= 83.04%

queen_honey_blossom answered 1 year ago

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