Benzoic acid Essays

Through the extraction process, the mixture was separated into its pure benzocaine and benzoic acid portions. This could be proven by matching the melting points of the substituents obtained at the end of the lab to the average melting points found in several chemistry databases. In other words, the melting points of the purified benzocaine and benzoic acid compounds (93.2˚C and 131˚C, respectively) reflect a similar melting points to the documented 89˚C and 122.41˚C of the pure compounds found in

benzaldehyde is 106.121g/mol, and the molar mass of benzoic acid is 122.12g/mol. With that in mind, to calculate the maximum possible mass of benzoic acid, which is the product of the experiment, Equation #2 must be used. Referencing from Table 1.1, the observed benzaldehyde mass is 5.02g, thus the plugging that into Equation #2, the calculation would be, (122.12 g⁄mol C_7 H_6 O_2)/(106.121 g⁄mol C_7 H_6 O)×5.02g, equaling to, 5.78g±0.01g of benzoic acid. To calculate the percentage yield, Equation #1

commonly used to synthesize benzoic acid. The importance of benzoic acid in modern world is due to its uses: the acid and its salts are used as preservatives in food: benzoic acid is globally known as E210 and sodium benzoate as E211. The benzoic acid and its precursors are also used in pharmacy and hygiene products : the shampoo and shower gel that I am using all contain sodium benzoate. With its increasing production I was curious to explore the synthesis methods for benzoic acid and try it in the laboratory

Abstract The unknown concentration of benzoic acid used when titrated with standardized 0.1031M NaOH and the solubility was calculated at two different temperatures (20◦C and 30◦C). With the aid of the Van’t Hoff equation, the enthalpy of solution of benzoic acid at those temperatures was determined as 10.82 KJ. This compares well with the value of 10.27KJ found in the literature. Introduction Solubility is a chemical property that is measured in terms of the maximum amount of solute dissolved in

Student’s Name Instructor’s Name Course Date Extraction Aim To separate a mixture of Benzoic acid, 4-t-butylphenol and Biphenyl and to determine the percentage recovery of each Theory Bicarbonate ions, when added to a mixture of the three substances, will convert the carboxylic acid (in this case, benzoic) to ions. Hydroxide ions on the other hand convert Phenols to ions. This makes them soluble in the aqueous layer as ions are soluble in water. However, addition of HCl to the aqueous ionic solutions

solid organic substance using a hot solution as a solvent. This method will allow the separation of impurities. We will analyze Benzoic Acid as it is dissolved and recrystallized in water and in a solvent of Methanol and water. Reaction/Summary In Experiment One we will be recrystallizing Benzoic Acid from water. In Experiment Two we will be recrystallizing Benzoic Acid using a solvent pair made up of Methanol and Water. The Seven step process of recrystallization consists of adding a solid organic

Moreover, these different phase diagram might be analyzed and compared individually in order to have a better understanding about the multiple types of phase equilibrium and phase change that occurs. For the procedure, the two components are benzoic acid and o-toluic acid. The first step of this experiment is to accomplish the part A: run samples A1 to A5 and B1 to B5. For this step, place a beaker of silicon oil on top of a hot plate until the temperature reaches 135 +/-

The Partition Coefficient (Kp) Excretion of Benzoic acid and its conjugate Base from Two Immiscible Phases Abstract: The partition coefficient is the ratio of concentrations of compounds in the two phases of a mixture of two immiscible solvents at equilibrium. The purpose of this experiment is to determine the partition coefficient of benzoic acid first in water with methylene chloride, and then in sodium bicarbonate solution with methylene chloride. The partition coefficient result for Part A (water

Procedure First, five standard solutions were made using 10-, 20-, 30-, 40-, and 50-mg/L of caffeine. The 10-mL solution was created by mixing 10-mL caffeine standard and 10.0-mL 0.10M HCl and diluting to 100.0-mL. This same procedure was used to make the rest of the solutions. Then 6.0-mL of soda, with the carbon dioxide removed, was placed in a 100-mL volumetric flask along with 10.0-mL 0.10m HCl and diluted. Then, the UV absorbance of the five standards was taken. Water was used in the reference

In this lab, extraction was used as a method for separating a mixture of compounds. Specifically, Benzocaine and Benzoic Acid were individually isolated from a starting mixture which consisted of both components. During this lab, Benzocaine was isolated into crystals, while benzoic acid formed a white powdery solid. This was done by first isolating benzocaine. Once separated, this clear liquid had 6M of sodium hydroxide added to it and was put in an ice bath. Once cooled, crystals formed. These crystals

Grishma Patel Chloroplast Pigments and Colored Light Absorption Summary The purpose of executing this lab was to see how different wavelengths and colors of light are absorbed by chloroplast pigments. The goal was to see the variations of light dependant reactions of photosynthesis based on different types of light. Spinach was used by grinding it with acetone and acquire the thylakoids used in the experiment. DCIP was used in this experiment as the oxidizing agent that will turn blue to clear when

the final product, benzoic acid and hydroxy magnesium bromide. In this reaction it is important to note that benzoic acid is not usually soluble in water, but deprotonating it tricks it into going into the aqueous layer. Also, we keep biphenyl (and the product) in the ether layer because biphenyl cannot be protonated or deprotonated.

- Medicinal Chemistry - Question No. 3. Define the Hammett Constant and the hydrophobic (Hansch) substituent constant. Comment on how inductive and mesomeric polar effects are treated in substituted aromatic systems. A quantitative structure-activity relationship (QSAR) is an equation which correlates measurable or calculable physical or molecular properties to some specific biological activity. Once this relationship has been determined, it is possible to predict the biological activity of related

isopropyl alcohol to dissolve the Benzoic Acid. We filled the evaporating dish, stirred, and then decanted the sample into a 140mL beaker with a stirring rod. This

Acid-Base Extraction and The Extraction of Caffeine from Tea Bags and Purification by Sublimation. Summary: The isolation of organic compounds in a solution can be performed due to the difference in solubility in different liquids. The extraction of the benzoic acid ,3-nitroaniline and 9-flourene mixtures by adding different amounts of solvents and extracting the acidic, basic and the organic solvents the purity of the samples were then determined by comparing them to the literature value of the

PChem Experiment No. 3 Cryoscopic determination of molecular weight 1. Aims To determine the apparent molecular weight of benzoic acid in cyclohexane by creating a binary system and finding the different freezing points of the solutions. 3. Experimental Procedure A dry, empty freezing-point tube and its cork were weighed together. Carefully, 15-20g of pre-cooled cyclohexane was poured into the freezing-point tube, the tube recorked, and the whole thing was reweighed, to find the exact mass of the

to water it was found that hexane which in non polar was semi soluble. The only soluble solvent was methyl alcohol which was detected after 20 seconds. When determining the solubility of malonic acid in different solvents both water and methyl alcohol were found to be polar when mixed with malonic acid. Hexane however was insoluble. Lastly biphenyl was mixed with water and was found to be insoluble, methyl alcohol was determined to be partially soluble.Hexane on the other hand was the only soluble

components of acid, base and neutral compound. The compounds were identified by melting point and matched up with the known melting points from a given list. In order to identify the compound it was important to separate by dissolving the mixture in an organic solvent which was not soluble in water, and then extracting the solution first with HCl, and then dilute sodium hydroxide solution. From the separation mixture, the aqueous layer were obtained and labeled as TT-1 (base), TT-2(acid) and TT-3 (neutral)

is not as likely). However, the reason that acetyl was not bound in the ortho position was because the para position demonstrated the least amount of steric hindrance. In other lab procedures, benzoic acid is sometimes substituted for anisole in the Friedel-Craft acylation. However, the reason benzoic acid

solubility of benzoic acid in the organic layer versus the aqueous layer. The partition coefficient is extremely useful in the health sciences due to the crucial information it gives for establishing proper drug delivery. Having precise drug delivery is vital for making sure pharmaceutical compounds are distributed in the body as safely and effectively as possible. In this experiment, a liquid-liquid extraction was performed in order to purify benzoic acid. In part A of this experiment, benzoic acid is dissolved