Technique and Theory of the synthesis of isopentylacetate?
Why is it easy to remove the excess?
1)It is water soluble and is removed during the water wash.
2)It is removed by deprotonation by the sodium bicarbonate solution.
3)The boiling point is very different and so it is removed during the distillation.
4) It is removed because it easily absorbs onto the sodium sulfate drying agent.
I think first one 1) is the answer.anyone agrees?I want to make sure.Thank you.
Answer:
Tne answer is B
Your product is an ester and your SM is an acid. If you deprotonate the acid, you'll make a water soluble salt and that can be readily separated from the product (which would not be very water soluble. If you do a 2 layer separation, you could recover the ester from the organic extract.
1) Use acetic anhydride or acetyl chloride, or
2) Remove the water with azeotropic distillation.
3) The ester has low water solubility. Wash the crude mixture with mild base to grab the HOAc as a salt in the aqueous phase.
Actually answers 1-3 are correct. A lot of the excess acetic acid can be removed by H2O washing. Any remaining can then be neutralized with NaHCO3. So answers 1 and 2 are correct. Answer 3 will also work since your product boils at 142 C and acetic acid boils at 118 C. If I were doing this procedure the first thing I would do to work up the reaction is first distill off as much acetic acid as you can using a rotary evaporator (this is a tool that normal labs have to remove solvent acetic acid included versus regular distillations). I would then dissolve the residue from the distillation in a solvent such as ethyl acetate. I would then wash this solution with H2O followed by a saturated NaHCO3 solution. Finally I would wash it again with H2O then with brine and dry it with sodium sulfate. I have done many reactions like this and what I have described is pretty much standard procedure. I hope this helps.
The answers post by the user, for information only, FunQA.com does not guarantee the right.
More Questions and Answers: