1. Write out the balanced equation for the reaction between salicylic acid and acetic
anhydride
.
2. Calculate the percent yield for the above reaction if the amount of aspirin
obtained was 2.301 g.
3. Calculate the theoretical yield of aspirin if you start with 2.687 g of salicylic acid
and an excess of acetic anhydride.
4. If you were to start with 1.00 g of salicylic acid, what volume of acetic anhydride
would be needed to completely react with it? The density of acetic anhydride is
1.082 g/mL.
5. According to your results from part 3 of this experiment, what can you say about
the purity of your aspirin? Be as specific as possible.
6. Explain why acetic acid is unlikely to be a contaminant in your solid aspirin.
7. Look up and record the boiling point of acetic acid, and explain why only some of
it evaporates from the reaction mixture.
8. If you measured the melting point of the solid product from this experiment and
obtained a melting range of 122-128 ℃, what does this tell you?
9. Aspirin that has been stored for a long time may give a vinegar-like odor and give
a purple color with FeCl3. What reaction would cause this to happen?
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