Acid Base Extraction Separation
da Alvarenga
Lab Partner: Keren Appiahene
Mussie Gide
10 September 2016
Experiment 2: Acid- Base Extraction Separation of an Organic Acid, a Base and a Neutral Compound
Introduction:
The extraction technique is often used in the organic lab to separate organic compounds from mixtures. One type of an extraction technique is the acid-base extraction, which is used to separate organic compounds from a mixture based on their acid-base properties.1 There are certain principles that must be taken into account when choosing a solvent system to perform an extraction. The solvents should not dissolve in each other. The solvents must have a favorable distribution coefficients (K) in order to be separated. The solvents must not react chemically …show more content…
The masses for the benzoic acid, 4- chloroaniline and naphthalene are as follow 2.890 g, 3.024 g and 3.036 g. The masses for the three products demonstrates that there was almost an equal amount of product that was extracted for each compound. The beginning mixture was 3.5 g which had equal amounts of the three compounds. Because the masses were close in range and they yield an average of 84.8 % percent recovery the experiment proved to be an effective technique of separating an organic acid, a base and a neutral compound. There could have been possible sources of error that occurred during the extraction process of the compounds because the percent recoveries were less than 100 %. Some possible reasons for a lower percent recovery are not properly drawing off the lower layers and extracting part of the top layer or leaving excess precipitate in the vacuum filter. Once the products were collected and weighed the melting point of each compound was recorded. The melting points for the acid, base and neutral compound are 100ºC, 81ºC and 75ºC. The melting point results are somewhat consistent with the literature values because the benzoic acid was lower than 122ºC while the 4-chloroaniline was within the range of 68-71ºC and the naphthalene was 5ºC lower than the expected melting point of 80ºC. A possible reason for the inconsistencies are the point at which the product turned to liquid was probably not properly
Lab Partner: Keren Appiahene
Mussie Gide
10 September 2016
Experiment 2: Acid- Base Extraction Separation of an Organic Acid, a Base and a Neutral Compound
Introduction:
The extraction technique is often used in the organic lab to separate organic compounds from mixtures. One type of an extraction technique is the acid-base extraction, which is used to separate organic compounds from a mixture based on their acid-base properties.1 There are certain principles that must be taken into account when choosing a solvent system to perform an extraction. The solvents should not dissolve in each other. The solvents must have a favorable distribution coefficients (K) in order to be separated. The solvents must not react chemically …show more content…
The masses for the benzoic acid, 4- chloroaniline and naphthalene are as follow 2.890 g, 3.024 g and 3.036 g. The masses for the three products demonstrates that there was almost an equal amount of product that was extracted for each compound. The beginning mixture was 3.5 g which had equal amounts of the three compounds. Because the masses were close in range and they yield an average of 84.8 % percent recovery the experiment proved to be an effective technique of separating an organic acid, a base and a neutral compound. There could have been possible sources of error that occurred during the extraction process of the compounds because the percent recoveries were less than 100 %. Some possible reasons for a lower percent recovery are not properly drawing off the lower layers and extracting part of the top layer or leaving excess precipitate in the vacuum filter. Once the products were collected and weighed the melting point of each compound was recorded. The melting points for the acid, base and neutral compound are 100ºC, 81ºC and 75ºC. The melting point results are somewhat consistent with the literature values because the benzoic acid was lower than 122ºC while the 4-chloroaniline was within the range of 68-71ºC and the naphthalene was 5ºC lower than the expected melting point of 80ºC. A possible reason for the inconsistencies are the point at which the product turned to liquid was probably not properly