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The image you've uploaded details a chemistry experiment focused on synthesizing aspirin (C₉H₈O₄) using salicylic acid (C₇H₆O₃) and acetic anhydride (C₄H₆O₃). The reaction also produces acetic acid (C₂H₄O₂) as a byproduct. Below is a breakdown of the key points from the text:

### Reaction:
\[ \text{C₇H₆O₃ (acide salicylique)} + \text{C₄H₆O₃ (anhydride éthanoïque)} \rightarrow \text{C₉H₈O₄ (aspirine)} + \text{C₂H₄O₂ (acide éthanoïque)} \]

### Protocol:
1. **Prepare a water bath at 70°C.**
2. **In an Erlenmeyer flask**, add:
   - 10.0 g of salicylic acid
   - 14.0 mL of acetic anhydride
   - A few grains of pumice stone.
3. **Gently heat the flask** in the water bath.
4. **Adapt a reflux system** on the flask.
5. **After 15 minutes**, place the flask in an ice bath.
6. **Let the reaction proceed** for 15 minutes, periodically extracting samples to monitor progress by chromatography (CCM).

### Chromatography:
- Used to monitor the progress of the reaction.

### Given dataThe image you've uploaded details a chemistry experiment focused on synthesizing aspirin (C₉H₈O₄) using salicylic acid (C₇H₆O₃) and acetic anhydride (C₄H₆O₃). The reaction also produces acetic acid (C₂H₄O₂) as a byproduct. Below is a breakdown of the key points from the text:

### Reaction:
\[ \text{C₇H₆O₃ (acide salicylique)} + \text{C₄H₆O₃ (anhydride éthanoïque)} \rightarrow \text{C₉H₈O₄ (aspirine)} + \text{C₂H₄O₂ (acide éthanoïque)} \]

### Protocol:
1. **Prepare a water bath at 70°C.**
2. **In an Erlenmeyer flask**, add:
   - 10.0 g of salicylic acid
   - 14.0 mL of acetic anhydride
   - A few grains of pumice stone.
3. **Gently heat the flask** in the water bath.
4. **Adapt a reflux system** on the flask.
5. **After 15 minutes**, place the flask in an ice bath.
6. **Let the reaction proceed** for 15 minutes, periodically extracting samples to monitor progress by chromatography (CCM).

### Chromatography:
- Used to monitor the progress of the reaction.

### Given 
- Density of acetic acid \(\rho = 1.082 \, \text{kg/L}\).

### Questions:
1. Calculate the molar masses of the reactants and products.
2. Demonstrate that acetic anhydride was added in excess.
3. Calculate the expected mass of aspirin in this synthesis.
4. Propose an experiment to ensure the synthesis is complete.
5. Explain how to confirm that the reaction is finished.

Would you like me to walk you through the calculations for any of the questions mentioned, or provide further explanation on the synthesis steps? Here are 5 related questions:

1. How is the excess of a reactant determined in a reaction?
2. What is the role of a water bath in chemical syntheses like this one?
3. How can the purity of the synthesized aspirin be tested?
4. Why is chromatography used during this reaction?
5. How would one calculate the yield of the reaction?

**Tip:** When calculating the theoretical yield of aspirin, always use the limiting reagent to ensure the correct mass is predicted.

Synthesis of aspirin using salicylic acid (C₇H₆O₃) and acetic anhydride (C₄H₆O₃), with acetic acid (C₂H₄O₂) as a byproduct. Tasks include calculating molar masses, determining reactant excess, and proposing experiments to ensure the completion of the synthesis.

Learn how to synthesize aspirin using salicylic acid and acetic anhydride. This guide includes stoichiometry concepts, molar mass calculations, and methods to confirm the reaction’s completion. Suitable for high school chemistry students.

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