Look up and record the boiling point of acetic acid, and explain why only some of it evaporates from
Answers
Answer:
Heating the mixture to a temperature above the boiling point of acetic acid, but below 100°C (the boiling point of water). The vapours from the acetic acid rise, and go into a tube. They are then condensed within the tube, and run off into a separate storage area. Because water can exist as a gas at pretty much any temperature above 0°C, it will result in an impure mixture, but repeatedly doing this will get the acetic acid to the desired purity.
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From: Ponyofishyinthec
Rewritten:me
Answer: (1) Explain why acetic acid is unlikely to be a contaminant in your solid aspirin. (2) Look up and record the boiling point of acetic acid, and explain why only some of it evaporates from the reaction mixture. (3) 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? (4) Aspirin that has been stored for a long time may give a vinegar-like odour and give a purple colour with FeCl3. What reaction would cause this to happen?