Question

1. Write out the balanced equation for the reaction between salicylic acid and acetic anhydride. 2. Calculate the percent yield step if you start with 2.687 g of salicylic acid with excess of acetic anhydride and the amount of aspirin obtained was 2.301 g. 3. Explain why acetic acid is unlikely to be a contaminant in your solid aspirin. 4. If you measured the melting point of the solid product from this experiment and obtained a melting range of 122-128 °C, what does this tell you? 5. Aspirin that has been stored for a long time and gives a purple color with FeCl3 (Tests for Functional Groups). What reaction would cause this to happen?

          1. Write out the balanced equation for the reaction between salicylic acid and acetic anhydride.

2. Calculate the percent yield step if you start with 2.687 g of salicylic acid with excess of acetic anhydride and the amount of aspirin obtained was 2.301 g.

3. Explain why acetic acid is unlikely to be a contaminant in your solid aspirin.

4. If you measured the melting point of the solid product from this experiment and obtained a melting range of 122-128 °C, what does this tell you?

5. Aspirin that has been stored for a long time and gives a purple color with FeCl3 (Tests for Functional Groups). What reaction would cause this to happen?

1. Write out the balanced equation for the reaction between salicylic acid and acetic anhydride.

2. Calculate the percent yield step if you start with 2.687 g of salicylic acid with excess of acetic anhydride and the amount of aspirin obtained was 2.301 g.

3. Explain why acetic acid is unlikely to be a contaminant in your solid aspirin.

4. If you measured the melting point of the solid product from this experiment and obtained a melting range of 122-128 °C, what does this tell you?

5. Aspirin that has been stored for a long time and gives a purple color with FeCl3 (Tests for Functional Groups). What reaction would cause this to happen?

Added by Christopher S.

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