Extraction of benzoic acid and naphthalene lab report. (DOC) Lab report 5 Extraction 2022-10-24
Extraction of benzoic acid and naphthalene lab report Rating:
The extraction of benzoic acid and naphthalene is a common laboratory procedure that involves the separation of these two compounds from a mixture using a solvent. This technique is often used in the field of chemistry to purify and isolate specific compounds for further analysis or for use in a chemical reaction.
To begin the extraction, a sample containing both benzoic acid and naphthalene is dissolved in a solvent such as dichloromethane or hexane. The solvent is chosen based on the relative solubility of the two compounds in the mixture. Once the sample has been dissolved, the mixture is shaken vigorously to ensure that the compounds are evenly distributed throughout the solvent.
Next, the mixture is filtered through a separatory funnel to separate the solvent from the solid mixture. The solvent, which contains the dissolved benzoic acid and naphthalene, is then collected in a flask. The remaining solid mixture is discarded.
The collected solvent is then washed with a small amount of an aqueous solution, such as water or an acid, to remove any impurities or contaminants. This step helps to purify the extracted compounds and improve the overall yield of the extraction.
After the solvent has been washed, it is allowed to evaporate, leaving behind the purified benzoic acid and naphthalene as a solid residue. The yield of the extraction can be calculated by weighing the purified compounds and comparing it to the initial weight of the mixture.
Overall, the extraction of benzoic acid and naphthalene is a useful laboratory technique that allows for the separation and purification of specific compounds from a mixture. This technique is commonly used in a variety of applications, including the analysis of chemical compounds, the preparation of samples for further experimentation, and the synthesis of new compounds.
Differences in solubility - intermolecular forces again AND a NEW IMF! The solution was swirled while the acid was being added to allow the carbon dioxide gas formed to dissipate. The given unknown sample will be dissolved with dichloromethane. Diethyl ether 1 pt. Immiscible liquids liquids that do NOT mix - intermolecular forces again! Copyright, Arizona State University Arizona State University: Organic Chemistry Lab Experiment Extraction Lab Package Separation and Purification 1. Rinse the beaker with 1 mL of deionized water and filter this also, trying to get as much of the solid as possible onto the filer paper.
The main goal this experiment was to succeed an acid-base reaction which helps to take out the benzoic acid during changes in solubility. To confirm the purity of the recrystallized naphthalene and benzoic acid, a thin layer chromatography TLC experiment was performed comparing the two pure compounds to the original mixture of the two. My main interests at this time include reading, walking, and learning how to do everything faster. After extraction of the benzoic acid into the aqueous solution as its anionic salt, the ether solution was then washed with water two further times. However, the file name should not be too long.
Leave the vacuum running, pulling air through the filter paper for at least 10 minutes to dry your crystals. Hydrochloric acid will then be added and extraction of p-nitroaniline will be performed in two steps: mixing and separation. Your handwriting should be neat and legible. The solubility of acids in different solvents depends on the ionization state. Anhydrous sodium sulfate will be added to the left over dichloromethane solution. Reaction if applicable 4.
Bases RNH2, like ethyl 4-aminobenzoate are protonated to form RHN3+. A few drops from the interface of the two layers were discarded each time to prevent contamination of the products. This percent recovery gained from this experiment was 86. At 80ºC the calibration curve was 3. This addition caused a white, solid benzoic acid to precipitate out of the solution.
SOLUTION: ASU Extraction and Purification of Naphthalene and Benzoic Acid Lab Report
This information is then applied to the procedure required for this experiment. As always, a lab coat should also be worn inside the lab. Seek immediate medical attention. A couple other obvious spots where error occurred were during vacuum filtration and decanting of the dichloromethane. The % recovered based on the mass of the teabags as a whole was 1. The dichloromethane layer was then transferred back to the original centrifuge tube again using the pipet.
What was the sign of the charge on the ionized benzoic acid, positive or negative? Conclusions: The purpose of this experiment was to separate a sample of benzoic acid, 2- naphthol, and naphthalene of unknown proportions. Link for Video of the Lab: Use these provided data below to complete your In-Lab in your notebook and your Postlab-Due at the end of your scheduled lab period time. However, there are endless numbers of possible mixtures, which make it impossible to have a pre-designed procedure for every mixture. The remaining organic layer is the naphthalene, which is also measured. The benzoic acid was allowed to air dry for a week. If you submit the file that is not readable by Canvas, a 10 point deduction will be applied to your lab report score. The reaction to extract the 2 base extraction reactions are performed in the chemical reaction below: Kugel, Morgan 1 Figure 1: The chemical Reaction Equations for both the Organic Base Extractions, Number 1 is Neutral to Ionic reaction while Number 2 is the Ionic to the Neutral reaction.
Give brief, 1- 2 sentence responses to the following questions: 2 pts. You can combine the weights of the chemicals you isolated and compare that weight to the weight you started with to determine a percent recovery. Dividing the mass of each of the isolated products by the total mass of the isolated products yields the percent composition of the recovered sample. In the Extraction experiment, liquid-liquid extraction was used to separate and purify naphthalene and benzoic acid from a mixture of the two through a separatory funnel. The lower layer of the mixture, the dichloromethane layer, was then transferred using the pipet into a clean centrifuge tube. How can you avoid this? Scroll to Section 2.
(DOC) Extraction of Benzoic Acid and Naphthalene in Mixture
In this instance, the naphthalene is soluble in ether, but insoluble in aqueous solution. The solid residue, naphthalene, was allowed to air dry for a week. Organic layer 1 pts. PRE-LAB: You must watch the online recitation, complete the GAPPED NOTES and also the NOTEBOOK PRE-LAB notes as summarized below. A sample comprised of a mixture of unknown proportions of benzoic acid, 4-nitroaniline p-nitroaniline , and naphthalene weighing 0. Pushing start temp lets you control the starting temperature. How can it be improved? Considering this, gloves and goggles should be worn when handling since the toxins can burn human skin.
Extraction of Benzoic acid and opportunities.alumdev.columbia.edu
With the use of pH, extractions can manipulate the solubility of different compounds so that they can be separated from a mixture. During the experiment, my lab partner and I did not completely mix the mixture of benzoic acid, 3-nitroaniline, and naphthalene with the DCM. Introduction In organic chemistry, the purification of reaction products and separation of immiscible liquids are achieved in both microscale and macroscale experiments. The benzoic acid will also be recrystallized using boiling water, and will then be weighed and measured for its melting point. Hello buddy, I have gone through your literature and compiled the laboratory report based on your initial instructions.
The dichloromethane solution which was allowed to stand was decanted into a clean test tube. In your extractions you will be using both an acid solution and a base solution. You will NOT BE ALLOWED TO PEFORM THE LAB if you have not completed ALL OF THE PRE-LAB activities, including the Experiment and Objectives worksheet, Section 4. The percent recovery is the percentage of the starting chemicals that you isolated. The naphthalene was weighed and transferred to a vial to dry for a week.