资料来源: Vy 先生和1月的里德尔, 加州大学欧文分校化学系
一个迪恩-斯塔克陷阱是一个特殊的玻璃器皿, 它允许收集水在反应通过一个共沸蒸馏。从反应中收集水的愿望可能有各种原因。它能驱动平衡在反应, 水被形成作为副产品。根据 Le 勒夏特的原理, 温度、压力、浓度或体积的变化将导致可逆反应的调整, 从而建立新的平衡。缩醛的形成是可逆反应, 水是作为副产品而形成的。在这种情况下, 通过移除水来达到产品侧的平衡, 可以获得良好的产量。院长斯塔克的陷阱也允许测定水的含量, 或者可以用来通过共沸蒸馏从溶剂混合物中除去水。
Water will form and becomes trapped over the course of the reaction. The theoretical amount of formed water upon complete conversion can be calculated and compared with the measured amount of the trapped water to determine the reaction progress.
This experiment demonstrates vividly Le Chatelier's principle and how it can drive an equilibrium.
Dean-Stark traps are commonly used to remove water from a solvent mixture under various circumstances. For example, the removal of water through a simple distillation when water does not form an azeotrope with the other solvent, is possible with a Dean-Stark trap based on its design. In the case of an azeotropic distillation, the addition of an entrainer is necessary. An entrainer is an organic solvent, which will form an azeotrope with water but does not mix with water in the liquid phase. The addition of an entrainer ensures the continuous removal of water, which becomes trapped in the side arm of the Dean-Stark trap. Unlike the Dean-Stark trap, a normal distillation apparatus requires the continuous addition of an entrainer since the distilled entrainer cannot flow back to the solvent mixture.
The Dean-Stark trap can also be used to drive the equilibria of reactions, where water forms as a byproduct, like in an ester or acetal formation. Through an azeotropic distillation where the solvent is also the entrainer, water is removed from the reaction and therefore from the equilibrium.
Finally, an azeotropic distillation with a Dean-Stark trap can also be used to determine the water content of solvents or solvent mixtures. Not only can water be removed with a Dean-Stark trap, but also volatile alcohols by placing 5-Å molecular sieves in the trap.
The Dean-Stark trap is used to shift the equilibrium of organic reactions to the product side.
According to Le Châtalier’s principle, an equilibrium can be driven toward the products using an excess of one of the reactants, by continuously removing one of the products, or by changing the temperature or the pressure at which the reaction is carried out. Perhaps the most commonly encountered equilibrium reactions are those involving water as a product.
As stated previously, the removal of this water can drive the reaction to completion. A Dean-Stark trap is a specialized piece of glassware used for continuously removing water formed in a chemical reaction.
This video will illustrate the principles of the Dean-Stark trap, a laboratory procedure in which the apparatus is used, and several applications.
Reactions such as the conversion of boronic acid to an ester result in the formation of water, which can hydrolyze the ester back to the acid, decreasing the overall yield.
As the reaction progresses, the water produced in the reaction may be continuously removed from the flask with the use of a Dean-Stark trap. In order to do that, first add the reaction components to a flask along with a hydrocarbon such as toluene and heat the mixture. As the reaction progresses, the water is released. Now toluene and water, which boil at 110 and 100 degrees, respectively, form an azeotrope, which boils at 84 degrees. Upon cooling in the condenser, the solvent vapors condense back to liquid, which drips into the collection vessel of the trap, and any overflow is returned to the reaction vessel.
The condensed liquid mixture eventually separates into two immiscible layers, with the denser component on the bottom. This is usually the water layer, which is then drained off. The same process is continued until no more water is produced, which indicates the completion of the reaction.
Now that we have discussed the principles of the Dean-Stark trap, let’s look at a laboratory procedure in which the apparatus is used.
In this procedure, we will react an aromatic aldehyde with ethylene glycol to yield an acetal protecting group, which shields the reactive aldehyde from further chemical reactions in a multistep synthesis. To begin, add to a 250-mL round-bottomed flask a stirbar, 7.5 g of 3-nitrobenzaldehyde, 75 mL of toluene, and ethylene glycol. Then attach the Dean-Stark trap to the flask and a reflux condenser onto the top of the trap.
Lower the flask and its contents in an oil bath, turn on the water in the condenser, and stir at 170 degrees. Allow the azeotropic mixture to condense and collect in the trap, and continue until the water formation ceases. After the two layers separate, measure the amount of water produced, and compare it to the theoretical yield. To verify the completion of the reaction, run the starting material and products on a TLC plate.
Once the reaction is complete, remove the flask from the heat source and allow it to reach room temperature. Discard the contents of the Dean-Stark trap, as they should not contain any product, and concentrate the contents of the flask under reduced pressure with a rotary evaporator.
To remove impurities, dissolve the yellow residue in 8 mL of hot ethanol and allow it to cool to room temperature, allowing the product to crystallize. Then, filter the solid, rinsing with cold ethanol, and dry it under vacuum.
Now that we have seen a laboratory procedure let’s look at some applications for which a Dean-Stark trap is used.
Enamines are substituted vinylamine compounds useful to form carbon-carbon bonds alpha to carbonyl groups. Enamines are prepared by heating a secondary amine, such as pyrrolidine, and an aldehyde or ketone, and removing the water byproduct with a Dean-Stark trap.
In addition to water, a Dean-Stark trap can be used to collect other compounds. Here, it was used to collect the product of an esterification reaction between benzoic acid and 1-butanol, which is also the reaction solvent. The 1-butanol is immiscible with and less dense than the product, and flows back into the reactor. The esterification product, which is hydrophobic, is also easily separated from the water byproduct.
An additional use for Dean-Stark traps is the determination of water content in foodstuffs. This is accomplished by placing a known amount of the food and boiling it in a hydrocarbon solvent. The volume of water collected from the distillate is measured, and divided by the weight of the food item to calculate the moisture percentage.
You’ve just watched JoVE’s introduction to Driving Equilibria with Dean-Stark Traps. You should now understand the principles of Dean-Stark traps, how to perform a laboratory procedure, and some of its applications. Thanks for watching!
