Acetic Acid Synthesis Lab Report

The average result obtained was 22.5% and is close to it’s literal value. This experiment had also proven to have shown effective transfer of solids and liquids as values of 1st and 2nd results, namely 22% and 23% respectively, were similar thereby showing consistency in results. Phenolphthalein indicator was proven to be more suitable as an indicator as compared to Methyl Orange in this experiment. This is because Phenolphthalein the pH values of HCl involved in this experiment were in range of the pH values that bring about colour change in the Phenolphthalein indicators. (Approximate pH ranges for color change: 8.0-9.8) Low pH values are preferred for Methyl Orange.

In addition, phenolphthalein was added as an indicator. The aliquots were titrated against sodium hydroxide (NaOH) solution until end point was reached, after which volume of NaOH consumed was recorded. The value of the rate constant, k, obtained was 0.0002 s-1. The experiment was then repeated with 40/60 V/V isopropanol/water mixture and a larger value of k = 0.0007 s-1 was obtained. We concluded that the rate of hydrolysis of (CH3)3CCl is directly proportional to water content in the solvent mixture.

This is because the amount of NaOH droplet can be altered when a burette is used thus, the NaOH solution can be dripped per drop at the time nearing the end point of the experiment as the colour changes rather quickly from light pink to pink. Conclusion: In conclusion, titration is an effective technique to determine the equivalence point, pH range, pKa, Ka and molecular mass of the unknown acid of the acid-base reaction. This technique is dependent on the colour change of the indicator which makes it easier to determine the end point of the experiment.

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

3. To purify and identify the product, recrystallization is used in order to purify the product, then melting point and TLC techniques are used to identify the product. Theory 4.

The ester studied was “3,” the acid used was 9.5 mL of “B,” and the alcohol used was 18.1 mL of “C.” A few substances were added to augment the production of the ester. Sulfuric acid (H2SO4) was added using a dropper bottle to catalyze the reaction. The desiccant in this reaction was drierite and was used to absorb the water byproduct. This prevented the ester from breaking apart into its constituents. The cold finger condenser was used to trap evaporated gas from the heated mixture, and condense it back into

Separation of Liquids by Fractional Distillation and Analysis by Gas Chromatography Methods and Background This lab was exceptionally knowledgeable and important in order to understand how certain compounds can be separated based on their boiling points (Landrie, 43). This experiment in particular focuses on understanding the separation of 1:1 mixture of acetone and 1 propanol using the method of fractional distillation (Landrie, 43). In the previous experiment, we focused on understanding the same separation but in terms of simple distillation. If compared with the data shown below with the data in the previous experiment, overall, the fractional distillation showed better and more effective results (Landrie, 43). This experiment also provided better

ABSTRACT The experiment aims to find the concentration of acetic acid in the vinegar sample by titrating it to a standardized NaOH solution, a base solution. A standardized 0.100 M NaOH solution was prepared from an available concentration of NaOH specifically a 1.00 M NaOH. The volume of the standardized solution (titrant) used which is 0.100 L was calculated using the M 1 V 1 = M 2 V 2 relationship.

The solvents that were used in this particular experiment included the likes of - n – hexane, Cyclohexane, cyclohexanol and Cyclohexyl acetate. Further they also reported the distribution coefficient and separation factors. When the two phase region was considered, n hexane and Cyclohexane proved to be suitable agents for establishment of equilibrium data of propionic acid-water-solvent mix. On the other hand, when distribution coefficient values were considered it was shown that Cyclohexyl acetate is most suitable. In conclusion, when all the properties were taken into consideration it could be concluded that cyclohexyl acetate is the most suitable extracting agent that was studied is this research.

Also, vitamin C is a necessary nutrient to humans; it is crucial to maintain the connective tissues and bones in the human body (Helmenstine) . Titration is a method that is used to determine the concentration of a solution by allowing certain volume of analyte to react with other concentration-known solution. It is important to know the point where enough titrant is added to react with the analyte, and this point is called the equivalence point. The equivalence point is shown by an indicator solution, which is a substance that changes color of the titrant at the equivalence point. However, in this experiment we are interested in finding the amount of titrant, rather than the equivalence point.

The objective of this experiment was the synthesis of Isopentyl Acetate using an esterification reaction between acetic acid and Isopentyl Alcohol, using a strong acid as a catalyst. The product was washed, and distilled. This approach is called Fisher esterification, whereby esters are produced by refluxing a carboxylic acid and an alcohol in the presence of a concentrated acid catalyst. The ester produced had a banana smell odor. The extraction of the crude product was conducted using sodium bicarbonate followed by distillation.

Purpose and Techniques: This experiment has the aim to determine a chemical formula of hydrated compound, which ingrains cupper, chloride and water molecules in its structure. In order to find this hydrated compound, it is necessary to use the law of multiple proportions. In other word, finding the appropriate variables values to this compound (CxCly*zH2O). Additionally, two major steps are required to proceed the experiment.

The difference in this chemical and physical properties will aid in their separation. Processes like solubility, gravitational filtration and recrystallization will be used to separate the substances present in Panacetin. The melting and boiling point of the substances will help in concluding on which of these compounds will be presented at the end of experiment. Procedure and observation The Panacetin content was weighed approximately 3.0493g and transferred to the Erlenmeyer flask; 75ml of dichloromethane (CH¬2CL2) was added to the content. The dichloromethane (CH2Cl2) dissolved the sucrose, leaving the active unknown agent and aspirin behind.

Name: University: Course: Date: Abstract I. Introduction/Motivation: The objective of this experiment was to characterize the behavior of a distillation column running in continuous mode. Two types of liquids were separated: 2-propanol and methanol (at 25 mol% and 75 mol% respectively).

The goal of this experiment was to synthesize the unknown ester through Fischer Esterification. This procedure involves treating a carboxylic acid with an alcohol and a strong acid catalyst. This procedure was also catalyzed with heat at 160oC-180oC, to keep the temperature from exceeding the boiling points of the compounds in use. The acid catalyst protonated the double bonded oxygen atom to force the atom to pull two electrons away from the double bond in order to stabilize the atom’s charge. As this electron shift occurred, the alcohol attacked the carbocation that lost its double bond.