1. Nonvolatile impurities
2. Another liquid boiling 25oC higher than the first liquid. They must dissolve in each other
In any distillation the flask should not be more than two-thirds full at the start. Great care should be taken not to distill to dryness because, in some cases, high boiling explosive peroxides can become concentrated.
Figure 5: Simple Distillation
Assemble the apparatus for simple distillation in the figure above starting with the support ring, followed by the electric flask heater and then the flask. One or two boiling stones are put in the flask o promote even boiling. Each ground joint is greased by putting three or four stripes of grease lengthwise around the male joint and pressing the joint firmly into the other without twisting. The air is thus eliminated and the joint will appear almost transparent. (Do not use excess grease as it will contaminate the product.) Water enters the condenser at the tublature nearest the receiver. Because of the large heat capacity of water only a very small stream (3 mm dia.) is needed; too much water pressure will cause the tubing to pop off. A heavy rubber band or a Keck clamp can be used to hold the condenser to the distillation head. Note that the bulb of the thermometer is below the opening into the side arm of the distillation head.
With distillation, we are able to separate the 1-bromobutane from 1-butene (side product) and inorganic salts, but other substances are in the same boiling point range as the product. However, all the three possible by-products (n-butanol, diethyl ether, and 1-butene) can be eliminated by extraction with concentrated sulphuric acid.
Extraction
Solvent extraction is the “pulling out” or removal of a substance from a liquid phase using another solvent.
It is also called liquid-liquid extraction. It involves the isolation of a pure solute dissolved in one liquid phase (usually aqueous) into an immiscible liquid phase (usually organic).
Solvent extraction is extremely useful for separations of a solute into another immiscible liquid before further qualitative or quantitative determinations. Hence, it is used to separate an analyte from interferences (or impurities) before determining the concentration of the analyte. In addition, solvent extraction is also used to isolate a product from a chemical reaction.
Washing and Extracting with various things
Now, getting back to extractions, there are really only four classes of compounds that are commonly handled in undergraduate extractions or washings.
1. Strong Acids. The mineral acids and organic acids (e.g., benzoic acid). You usually extract these into sodium bicarbonate solution or wash them with it.
2. Really weak acids. Usually phenols, or substituted phenols. Here, you'd use a sodium hydroxide solution for washing or extraction. You need a strong base to work with these weak acids.
3. Organic bases. Any organic amine (aniline, triethylamine, etc.). As you use bases to work with acids, use a dilute acid (5 to 10% HC1, say) to extract or wash these bases.
4. Neutral compounds. All else, by these definitions (e.g., amides, ethers, alcohols, hydrocarbons).
Steps of Extraction (Pictorial)
2. Shaking the separatory funnel to allow the two layers to mix
3. Allow the phases to separate out and collect the phase desired
1. Adding organic and aqueous phase into separatory funnel
After the final extraction, the organic phase is usually treated with a solid drying agent (eg. Sodium sulphate and sodium chloride) to remove traces of water, and then filter to remove the dehydrating agent. The excess organic solvent is evaporated off using rotary vaporizer, remaining behind a purified and concentrated solute.
Figure 6: List of drying agents
In this Experiment
After the distillation, the sample collected in the receiver contains 1-bromobutane and water containing some sulphuric acid, 1-butene, unreacted 1-butanol, and di-n-butyl ether.
By adding the concentrated sulphuric acid into the separatory funnel it will be able to remove any unreacted starting material as well as any alkenyl or ethereal byproducts. By the means of protonating or converting the byproduct to alky hydrogensulphate (details are provided in discussion)
Allow the two layers to separate completely and then remove the sulfuric acid layer. Washing the 1-bromobutane layer with Sodium Bicarbonate will allow us to remove traces of acid.
Dry the cloudy 1-bromobuatne by adding anhydrous CaCl2 and mixing until the liquid clears and no longer clumps together.
Procedure
3 Procedure
3.1 Reaction Setup
3.1.1 Foremost, we have transferred 30ml of deionised water into a 250ml rbf using a measuring cylinder.
3.1.2 The rbf was placed into an ice-bath to be cooled, 35 ml of concentrated sulphuric acid was added while swirling the rbf. This was to prevent the oxidation of bromide (added later) to be bromine which is useless in this experiment.
3.1.3 25ml of n-butyl alcohol was added into the cold diluted acid using a measuring cylinder, while ensuring thorough mixing and sufficient cooling.
3.1.4 35.7g powdered potassium bromide was weighted out and added into the reaction mixture while swirling the rbf to prevent formation of lumps. We had to ensure that the filter funnel used for the transfer of KBr was clean and dry to minimize the residual KBr on the wall of the funnel.
3.1.5 5-6 anti-bumping chips were introduced into the rbf to enable throughout distribution of heat and prevent violent boiling during the 30 mins reflux. We had to wipe the bottom of the rbf to keep the water from entering the heating mantle as that might spoil the heating mantle.
3.1.6 Next, we adjusted the heating so that the mixture may boil gently and the mixture was swirled cautiously from time to time.
3.2 Crude Purification using Distillation
3.2.1 We allowed the flask to cool for 5 mins and deionized water was introduced from the top of the condenser to wash down the condensate. Without delay, we have re-arranged the apparatus for distillation.
3.2.2 The reaction mixture was distillated at 105oC for 15-20mins and we have collected the distillate for solvent extraction and discarded the pot residual.
3.3 Crude Purification using Extraction
3.3.1 The distillate and about 25ml of deionised water was transferred into the separatory funnel, stopper tight and shake thoroughly while releasing the pressure every 2-3 secs. We have to ensure that when we release the pressure, the separatory funnel is tilted up and gradually release the pressure to prevent product losses.
3.3.2 Next, we removed the stopper and placed the separatory funnel on the retort ring to allow the atmospheric pressure to separate the organic and aqueous phase.
3.3.3 We have drained the organic layer into the conical flask and poured the inorganic phase into another conical flask from top of the separatory funnel. It is advisable to keep the aqueous phase in the case of product recovery.
3.3.4 12.5ml of 80% cold suphuric acid was carefully poured into the organic layer in the seperatory funnel.
3.3.4 Next, we have extracted the organic layer again with 15ml of saturated sodium hydrogencarbonate to neutralize and remove the acid into the aqueous phase in the same separatory funnel.
3.3.5 The final product was washed with 25ml water in same separatory funnel (similar to the first extraction process). The 1-bromobutane was drained into a clean and dry conical flask.
3.3.6 Anhydrous calcium chloride (to remove excessive water from organic phase) was added into the crude product and swirled gently to mix and stopped adding when we observe the CaCl2 to be able to fly around freely in the solution.
3.3.7 The dried product was filtered into a weighed measuring cylinder by gravity filtration to remove the CaCl2 from the 1-bromobutane.
3.3.8 The volume of the product was measured and weigh on a analytical balance. Hence, we are able to determine the yield and the density of the product.
Results and Calculations
4. Results and Calculations
4.1 Table of Reactant
Reaction Scheme
Yield of 1-bromobutane
=
=
= 57.1%
Density of 1-bromobutane
=
=
g/cm3
= 1.26g/cm3 (actual density = 1.2758g/cm3 from CRC handbook)
Discussion
5. Discussion
Mechanism of Reaction:
Reaction
In this experiment, SN2 nucleophilic substitution was carried out. Firstly, KBr reacts with sulphuric acid to give us Hydrogen Bromide which was used to protonate the hydroxyl group (strong base, poor leaving group) to give us water(weak base, good leaving group) as the leaving group. The -Carbon was attacked by the Br- (Nucleophile) on the backside as the leaving group leaves the -Carbon at the same time, since the cleavage of the C-H2O bond and the formation of C-Br takes place simultaneously, this reaction is known to be concerted.
Despite the pivotal role of HBr in the reaction, it was not added as one of the reactant. This is because pure HBr exists in gaseous form, making them difficult and hazardous to transport Jim C., 2002). Thus HBr is frequently, and in this experiment, produced in situ by adding potassium bromide to concentrated sulphuric acid, which protonates the bromide ion to form hydrobromic acid (Eve, 2011).
However, we have to ensure that the sulphuric acid is cooled and have to add the potassium bromide slowly as it might cause significant oxidation of potassium bromide to form bromine which will be rendered useless in this experiment and reducing our yield. Below are the equations:
KBr (s) + H2SO4 (aq) → HBr (aq) + KHSO4 (aq)
2 HBr (aq) + H2SO4 (aq) → Br2 (g) + SO2 (g) + 2 H2O (l)
Along with this reaction by-products such as n-dibutyl ether and but-1-ene were formed.
The strong acid causes the dehydration of n-butanol forming n-dibutyl ether and the mechanism is shown below:
The strong acid also causes the dehydration reaction of n-butanol and formation but-1-ene under E2 mechanism as shown below:
Liquid-Liquid Extraction
Therefore, it is essential for us to factor in by-products present into the crude purification process to isolate the 1-bromobutane. The flowchart below summarizes the crude purification process:
The Alkene, when passed through cold, concentrated sulphuric acid result in formation of alkylhydrogen sulphate (ester of sulphuric acid) as the addition product (Metha, 2005). The addition is regioselective and follows Markovnikov’s rule:
Ethers on reaction with hot sulfuric acid, form alcohol and alkyl hydrogen sulphate, however, in cold acid (in our case), the dibutyl ether could at least be protonated and thus soluble in aqueous.
Reaction under hot sulfuric acid:
Reaction under cold sulfuric acid (More relevant to our extraction):
N-butanol was protonated by the conc. Sulfuric acid and makes it soluble in aqueous sulphuric acid layer:
Percentage Yield and Density
The percentage yield of 1-bromobutane is 57.1% which is considerably low as the yield could be as high as 70%. The density of 1.26g/cm3 was obtained from this experiment is near the actual density of 1.2758g/cm3 stated in CRC Handbook this implies that the product is rather pure. However, we will not be able to confirm its structure until we carry out refractive index, 1HNMR or COSY.
Figure 7: 1HNMR Spectrum of 1-bromobutane (Chemdraw)
The low percentage yield of the sample may be due to several reasons. Firstly, there will be product losses in the aqueous phase of the series of extraction and during the transfer of product which is inevitable. For instance, during decanting, small amount of 1-bromobutane sample might have been discarded. This is because as the volume of the aqueous solution declines, the difficulty in ensuring that the organic layer is not discarded increases (Organic Chem Online, 2011). This small volume of 1-bromobutane that was discarded by accident will result in a lower percentage yield. However, we can reduce the product losses if we are cautious and careful during the extraction process and product transfer.
Secondly, side reactions have to be taken into consideration as they take up a sizeable amount of n-butyl alcohol from the reactants. Side products of this reaction include but-1-ene and butoxybutane, both which requires n-butyl alcohol as a reagent, thus, lowering the amount of n-butyl alcohol left to react with hydrobromic acid and eventually the product and percentage yield (University of Colorado, 2011).
Nevertheless, we may extend the time of the reflux reaction to maybe 45mins or 1 hour which will help to increase the yield by around 1-2 % (Kenneth L.Williamson, 2011). Moreover, we may also monitor the reaction with TLC by using co-spot, to estimate the amount of limiting reagent(LR) left in the reaction mixture (in this case is n-butanol) before carrying distillation. If the reaction is still incomplete, we can add more equivalent of KBr and acid to push the reaction forward as the rate of the reaction is dependent of the Br-.
Figure8: Co-spot TLC indicates not much limiting reagent,
n-butanol (more polar than 1-bromobutane) left in the RM (Chemdraw)
Lastly, the distillation process may be incomplete. In this experiment, the distillation process was carried out at 105oC; the main purpose of the distillation process would obtain 1-bromobutane from the reaction mixture and leaving excess n-butyl alcohol as pot residue. The boiling point of water and 1-bromobutane is 100oC (Elmhurst College, 2003) and 101.4oC respectively (Oxford University, 2003). The boiling point of n-butyl alcohol, on the other hand, is 118 oC (Oxford University, 2010). The large difference in boiling point between n-butyl alcohol and the product, 1-bromobutane is due to the ability of n-butyl alcohol to participate in hydrogen bonding (Jim C., 2006). This difference in boiling point allows water and 1-bromobutane to be separated from n-butyl alcohol. However, incomplete distillation may have occurred, resulting from the termination of the process before 1-bromobutane has been fully obtained. Incomplete distillation lowers the yield of the product as they are left behind and discarded, although this could be easily avoided by simply extending the time of the distillation process (Palmer R., 1918).
However, a more sensible option would be introducing a "chaser" solvent such as para-xylene (para-dimethylbenzene) to 'chase' away any remaining 1-bromobutane from the distilling flask. In our case, we might expect p-xylene (B.P. 138.4°C) to be a really good chaser, or pusher, for 1-bromobutane boils at 101.3°C.
A chaser solvent or pusher solvent is sometimes used to help blast our compound off the surface of the packing material. It should have a tremendously high boiling point relative to what we were fractionating. After we have collected most of one fraction, some of this material is left on the column. So, we throw this chaser solvent into the distillation flask, fire it up, and start to distill the chaser solvent. As the chaser solvent comes up the column, it heats the packing material, your compound is blasted off the column packing and more of your compound comes over. Stop collecting when the temperature starts to rise—that is the chaser solvent coming over now.
Lastly, if time permits, we can consider carrying out distillation purification after the extraction as this will help to increase the purity of our compound.
Conclusion
6. Conclusion
From the experimental result, the percentage yield of 1-bromobutane and density were also obtained which are 57.1% and 1.26 g/cm3 respectively. Therefore, we have managed to accomplish the aim of synthesizing 1-bromobutane under reflux setup and carry out crude purification with distillation followed by a series of extractions.
References
References
Books
James W.Zubrick. 1988. The Organic Chemistry Lab Survival Manual. Canada: John Wiley & Sons.
Fieser Williamson. 1992. Organic Experiments. Canada: D.C Health and Company.
Kenneth L.Williamson, & Katherine M.Masters , (2011) Macroscale and microscale organic experiments.. : Brooks/Cole.
Mehta, Bhupinder, & Manju Mehta, (2005) Organic Chemistry. New Delhi: Prentice Hall of India.
.
Internet
Houghton, M (1994) The SN2 Reaction: 1-Bromobutane PSU Chemistry, Available: http://courses.chem.psu.edu/chem35/Syn%20Sp06/35Exp140.pdf Last accessed 11th February, 2012
Preparation of 1-bromobutane Rodspages, Available: http://www.rod.beavon.clara.net/bromobutane_prep.htm Last accessed: 11th February, 2012