To determine how many ml of acetic anhydride are needed to produce 49.4 grams of aspirin, we begin by looking at the reaction involved in aspirin synthesis. The chemical reaction typically involves acetic anhydride and salicylic acid. The molar mass of aspirin (acetylsalicylic acid) is approximately 180.16 g/mol.
First, we calculate the number of moles of aspirin we want to produce:
Number of moles of aspirin = (mass of aspirin) / (molar mass of aspirin)
Plugging in the values:
Number of moles of aspirin = 49.4 g / 180.16 g/mol ≈ 0.274 moles
Next, the reaction stoichiometry indicates that 1 mole of acetic anhydride produces 1 mole of aspirin, meaning we need 0.274 moles of acetic anhydride.
The molar mass of acetic anhydride is about 102.09 g/mol. To find the mass of acetic anhydride required, we use:
Mass of acetic anhydride = (number of moles) x (molar mass)
Calculating the mass:
Mass of acetic anhydride = 0.274 moles x 102.09 g/mol ≈ 27.95 g
Now, we convert the mass of acetic anhydride to volume using its density (1.082 g/ml):
Volume (ml) = Mass (g) / Density (g/ml)
So the volume required is:
Volume = 27.95 g / 1.082 g/ml ≈ 25.9 ml
In conclusion, to produce 49.4 grams of aspirin, you will need approximately 25.9 ml of acetic anhydride with a density of 1.082 g/ml.