Benzoic acid

ether. The unknown was chosen from a predetermined list of benzoic acid derivatives with varying molecular weights and melting points (see Supplement C). The second purpose of this lab was to prepare an unknown carboxylic acid by reacting the unknown aryl-magnesium bromide with carbon dioxide and diethyl ether then protonating.The third purpose of this lab was to determine the neutralization equivalence point of the unknown carboxylic acid by titrating with sodium hydroxide. The fourth purpose of

Objective: The objective of this experiment is to use acid-base extraction techniques to separate a mixture of organic compounds based on acidity and/or basicity. After the three compounds are separated we will recover them into their salt forms and then purify them by recrystallization and identify them by their melting points. Procedure: Extraction of Carboxylic Acid A pre-weighed (0.315g) mixture of Carboxylic acid, a phenol, and neutral substance was placed into a reaction tube (tube 1)

moulds (Food Today 2004). Commonly used food additives Monosodium glutamate –for enhancing the flavour however it is a harmul additive as it contributes to weight gain Sodium Cyclamate –artificial sweetener Sodium Benzoate-prevent oxidation of fats Benzoic acid-in fruit juices stronger against bacteria than on yeasts and mould Sulfites-for stopping fermination Nitrites and nitrates-for colour retention and inhibiting growth of bacteria Antibiotics-given to food

Organic Lab I No. 5-6 Separation of a Carboxylic Acid, a Phenol, and a Neutral Substance (Two-week lab) Reading Assignment 1) Chapter 7 • Introduction: P. 135- first paragraph • Theory and Techniques (p142-145) o Properties of Extraction Solvents o Mixing and Separating the Layers o Drying Agents o Part 1: The Technique of Neutral Liquid/Liquid Extraction The description is for dichloromethane-aqueous

2-((2-aminoethoxy)methyl)-4-(4-chlorophenyl)-1,4-dihydro-6-methylpyridine-3,5-dicarboxylate Aripiprazole n-oxide 7-{4-[4-(2,3-dichlorophenyl)piperazin-1-yl]butoxy-n-oxide}-3,4-dihydroquinolin-2(1H)-one. Aspartane Impurity-A 2-(5-benzyl-3,6-dioxopiperazin-2-yl)acetic acid. Atenolol Impurity-A 2-(4-hydroxyphenyl)acetamide Atenolol Impurity-B 2-(4-((oxiran-2-yl)methoxy)phenyl)acetamide

The cloudiness is caused by the protonation of the sodium salicylate to salicylic acid which insoluble in the water. 3. A) Some of the counterfeit pharmaceutical would not dissolve so lowering percentage yield, purity, percentage composition of every component and the recovery of aspirin and the unknown as sucrose is too high. B) Sucrose

Alterations: After mixing the benzoic acid, p- dichlorobenzene, and m- nitroaniline with the diethyl ether inside the separatory funnel it resulted a yellowish color with a strong odor that makes you dizzy. Preparing an hydrochloric acid solution and mixing it with the mixture of diethyl ether and there three compound creates a layer in the separatory funnel. Shaking it and releasing the gas to mix the compound very well, but too much shake trap the bubbles in the center layer that separate the organic

various techniques can be used such as sublimation, evaporation, extraction, filtration, decantation, and more. In this lab, benzoic acid, benzocaine, and 9-fulorenone were mixed and acid-base extraction, separatory funnel extraction, drying organic solutions, suction filtration, and melting point determination were used to separate the mixture in to more pure substances. For the acid-base reaction, proton transfers occurred to result in compound polarity shifts, which allowed

Lab In this lab, we learned about the dissociation of acids through various tests between the acid, benzoic acid (C₇H₆O₂), and the acid-base indicator, phenolphthalein. When an acid dissociates, it gives it’s H+ particle to a base in need (usually with a formal negative on an oxygen). We found the use of heat and cooling and the factor of time as the main factors affecting the dissociation of acids in this experiment. The dissociation of acids produced visible changes in our test tube such as warmth

was added to benzoic acid. The half titration point is more difficult to determine based on the graph because there was an error in mixing the initial volume of base to acid. It is estimated that the half-equivalence point is when 3 mL of NaOH was added, giving a pH of 4.68. At the half-equivalence point, the is equal to the pKa, so it can be assumed that the pKa of benzoic acid is 4.93. b. At the half-equivalence point, the moles of based added has neutralized half of the moles of acid in solution