ipl-logo

Bromination Of Acetanilide And Aniline Lab Report

603 Words3 Pages

The objective of this lab was to perform halogenation reactions where acetanilide and aniline were brominated. The bromination of acetanilide can results in two possible products: 4-bromoacetanilide and 2-bromoacetanilide. Therefore, the melting point was used to confirm that 4-bromoacetanilide was formed and not 2-bromoacetanilide from the bromination of acetanilide. The bromination of aniline resulted into 2,4,6-tribromoaniline. At the end of the experiment, the mass of each bromination was determined to measure the reaction’s efficiency by calculating the percent yield. In addition, the melting point was measured to compare with the literature value and determine the purity of the final product. The bromination of acetanilide was performed …show more content…

From this reaction, only 0.113g (94.9% yield) of 4-bromoacetanilide was collected. When the solution was transferred to the Buchner funnel, some product got stocked in the small tube. The spatula was used to get the most of the mas of final product. Losing this small amount of the product caused the decreasing of the percent yield. By taking the melting point of this solution, it was confirmed that 4-bromoacetanilide was only formed. According to Chemspider website, 4-bromoacetanilide has a melting point of 165°C – 169°C (1) and 2-bromoacetanilide has a melting point of 96.5°C – 100.5°C (2). The melting point range of the experimental mass was 166.1°C – 168.1°C. This melting point was in the range of the literature value which confirmed that 4-bromoacetanilide was only produced and it was pure. From the bromination of aniline, only 0.203g (88.3%) of 2,4,6-tribromoaniline was collected at the end. In the same way, some mass was lost when the solution was poured into the vacuum because residues of mass were left inside the small test tube. This caused the decreasing of the percent yield. According to the website Sigmaaldirich, the melting point range for 2,4,6-tribromoaniline is 120°C – 122°C (3). The experimental melting point of the bromination of aniline was 119.8°C – 121.1°C. This small range in the melting point matched with the literature value which confirmed that the mass was

Show More
Related
382 Words | 2 Pages

Nevertheless, the latter is not used in this experiment since it is very reactive and extremely flammable. On the contrary, NaBH4 is relatively mild and it can be used with protic solvents. In this manner, 1.507 grs of the ketone 9-fluorenone were mixed with 30.0 ml of 95% ethanol in a 125 ml Erlenmeyer flask. The bright yellow mixture was stirred during 7 minutes until all the components were dissolved.

Read More
779 Words | 4 Pages

The following lab period the solid was weighed (0.0483 g) and percent yield was calculated (65.5%) with the limiting reagent being tetraphenylcyclopentadienone. The melting point was determined. The first melting point was 204-204.9 °C and the second melting point was 215.6-215.9°C. Finally, an infrared spectroscopy was obtained for the

Read More
904 Words | 4 Pages

9. The melting point range was lower than the given range of the anti-addition product by 2 degrees Celsius. This could have been due to impurities in the product. A likely cause could have been water that still remained in the product after recrystallization (the product shifted upward during melting point analysis due to evaporation). Since water has a low melting point, it could have lowered the melting point range of the product.

Read More
1039 Words | 5 Pages

The data table provided below obtained melting point data for crude product, pure product, and mixture of the pure and 4-tert-butylbenzyl. 12. The TLC data obtained is provided in a table below. The TLC data was conducted solely in a 9:1 hexane/ethyl acetate solvent solution as opposed to the 1:1 and pure hexane solution as well. This was due to the lack of time, but as explained in number 7, a very polar solvent (1:1 solution) or non-polar solvent (pure hexane) is not ideal when obtaining

Read More
912 Words | 4 Pages

5-aminotetrazole monohydrate: In a 250 ml round-bottom flask equipped with a condenser for refluxing (90 °C) and a magnetic stirring bar, 5.00 g (5.95 mmol) dicyandiamide (three times crystallized), 7.47 g (11.9 mmol) sodium azide and 11.00 g (17.8 mmol) boric acid and 100 ml of water is added and allowed to reflux for 24 hours, after the completion of the reaction, until the solution pH to about 2 to 3 as hydrochloric acid 37% is added (about 12 ml) Then the reaction mixture was cooled in a refrigerator for 18 hours and the white crystals formed. The mixture was filtered and washed three times with 10 ml of water and and dried in 60 °C for 5 hours and finally 45.8 g of product by it will be obtained. 5-Aminotetrazol monohydrate:

Read More
1445 Words | 6 Pages

Fluorene was precipitated when the sodium sulfate solution was added to the organic layer. As a result, the solubility of fluorene was decreased further when it was placed in an ice-water bath. Fluorene could also be obtained using vacuum filtration and 1,4-dibromobenzene remained in the fluorene solution due to its higher solubility. As it was 10% of the whole mixture, it is considered to be 1,4-ibromobenzene was the minor product and thus could be rejected. The melting point range was used to identify the unknown solids from the mixture.

Read More
872 Words | 4 Pages

In this particular lab, the insoluble barium iodate Ba(IO3)2 is produced by the reactants barium chloride and potassium iodate. the balanced equation to produce insoluble barium iodate is Ba^2+(aq)

Read More
565 Words | 3 Pages

The experimental melting point was calculated to be 159.0-159.6°C, which is very accurate compared to the actual melting range of 160-163°C. The percent yield came out to be 26.89%, which is low but is consistent with other in the class due to the difficult nature of forming the trimethylmethanol crystals. Overall, this was a successful experiment because in the end there was a decent amount of pure crystal product. Questions 1.

Read More
746 Words | 3 Pages

Once the bromine was added to each test tube, the color of each test tube was monitored, and the time that a color change occurred in each test tube was noted. Bromine is red; when the solution was no longer red, it could be understood that the reaction had taken place. For the test tubes exposed to UV

Read More
1111 Words | 5 Pages

In this test, primary halides precipitate the fastest while secondary halides need to be heated in order for a reaction to occur. Comparison of the rates of precipitation of the obtained product to standard 1° and 2° bromide solutions will show whether the product is a primary or secondary

Read More
1478 Words | 6 Pages

RESULTS AND DISCUSSION Preformulation Studies The melting point of Metoprolol Tartrate was determined by capillary method and was found to be 121ºC (120 - 124ºC) as reported in literature, thus indicating purity of Metoprolol Tartrate. FTIR analysis showed that all the characteristic peaks of Metoprolol Tartrate and mixture of Metoprolol Tartrate with excipients were present in the range of reported frequencies; which shows that drug and excipients were compatible with each other. DSC thermogram of Metoprolol Tartrate alone showed endothermic peak at 120.73°C, corresponding to the melting point of the drug. The thermal curve of the Metoprolol Tartrate obtained indicated its crystalline anhydrous state, exhibiting a sharp endothermic peak at 120.73°C.

Read More
502 Words | 3 Pages

A drying tube with calcium chloride was used for the reaction during the set up because it will remove and catch specific compounds leaving the reaction or being produced from the reaction. The purification method is by using adding petroleum ether to produce crystals and then vacuum filtration to remove the crystals from the solution. The melting point for 4-cyclohexene-cis-1,2-dicarboxylic anhydride as a pure compound is measured at approximately 97-103ºC. The measured melting point from the experiment is approximately 70-80ºC. The difference between the melting point temperatures can have been caused by excess xylene or water in the

Read More
1305 Words | 6 Pages

For this experiment, the pure products appear to be in the first and fifth fractions because these fractions had stabilizations of boiling points whereas the other fractions featured comparatively larger boiling point ranges. However, it is important to note that the second fraction had a significantly larger volume than the rest of the fractions did, and only a 4C temperature range reading. This suggests that there could have been some pure product in the second fraction as well, especially because the temperature range was increasing slowly until about 3 mL of distillate had been collected, and then it thermometer readings increased rapidly. The data for this experiment would have been more comprehensive if the after these 3 mL had been collected, a new fraction had been collected with the distillate from the more rapidly increasing temperature range reading had

Read More
938 Words | 4 Pages

The melting point of the experimentally synthesized Aspirin product was found to be between 126-129 ˚C. This temperature range of initial to final melting point has a small and sharp temperature range of only 3˚C, which is within the acceptable limits of the 128-137˚C1 literature value for Aspirin (Acetylsalicylic Acid/2-acetoxybenzoic acid), if located slightly toward the beginning of the literature melting temperature range. Therefore, the narrow melting point range, which falls within the standard literature value range results, indicate the reliability purity of the sample. Had the melting point been higher than the literature value, but maintained a sharp melting point range, the compound could have still indicated a pure sample. A lower

Read More
702 Words | 3 Pages

Firstly, unknown B has a low melting point, a prominent characteristic among covalent compounds. This is due to the attraction between the atoms not being as reinforced as an ionic compound, thus it takes less energy to separate. In addition, unknown B has a very low solubility and conductivity, this is due to the atoms sharing electrons, therefore they cannot have the ability to separate and form an ion. However, it should be noted that covalent compounds should most definitely not be conductive or soluble, but the results have shown otherwise, thus it should be concluded that there may have been contamination between the scoopula’s used. Conclusion

Read More

More about Bromination Of Acetanilide And Aniline Lab Report

Open Document