was mixed with glacial acetic acid and stirred in which then bromine/acetic acid solution was added to the mixture little by little. The dibromide becomes the precipitate of this solution during the reaction. Once this precipitate is separated by vacuum filtration the melting point helps identify the product. Laboratory notebook reference: Pages 9-10 Chemical Reactions: [pic] Observations: The experiment was begun by mixing trans-cinnamic acid and glacial acetic acid with an added stir
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weak acid: acetic acid‚ CH3COOH. • • • • • a strong acid: hydrochloric acid‚ HCl. an acidic commercial cleanser. a basic commercial cleanser. to use the titration curves to calculate the percent of the active ingredients in the commercial cleansers. to determine the Ka of a weak acid. Procedure Overview • • • • after calibration of the pH electrode and determination of the flow rate for the automatic titration‚ a NaOH solution is standardized against HCl. a pH titration curve for acetic acid is obtained
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hardness of bone is due to calcium deposits in the matrix while the flexibility comes from the organic material of the matrix. We can illustrate these facts by treating two bone samples by two different methods: 1. Soaking a bone in vinegar (dilute acetic acid) removes calcium and other minerals from the bone. Samples treated in this manner remain flexible but lose their hardness. 2. Baking a bone chars the organic material in the bone matrix leaving the bone very brittle. In this experiment we will
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buffer system consisting of solution of acetic acid and sodium acetate (CH3COOH/CH3COONa). CH3COOH --- H+ + CH3COO– CH3COONa ---- Na+ + CH3COO- since the salt is completely ionised‚ it provides the common ions CH3COO– in excess. The common ion effect suppresses the ionisation of acetic acid. This reduces the concentration of H+ ions which means that pH of the solution is raised. Thus‚ a 0.1 M acetic acid solution has a pH of 2.87 but a solution of 0.1 M acetic acid and 0.1 M sodium acetate has a
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Purpose 13C: 1. To titrate a hydrochloric acid solution of “unknown” concentration with standardized 0.5M sodium hydroxide. 2. To titrate a hydrochloric acid solution of “known” concentration with standardized 0.5M sodium hydroxide. 3. To titrate an acetic acid solution (vinegar) with standardized 0.5M sodium hydroxide. 4. To utilize the titration results to calculate the molarity of the hydrochloric acid and the molarity and percent composition of the vinegar. Hypothesis 13G: N/A Hypothesis 13C: N/A
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C6H5COOH + NaHCO3 C6H5COONa + CO2 + H2O H C6H5NH2 + HCl → C6H5N+H3Cl- 3. On the basis of solubility behaviour‚ determine the best solvent to differentiate the following pairs of compounds. a. CH3COOH (acetic acid) and CH3(CH2)5COOH The best solvent to use to differentiate acetic acid from heptanoic acid would be sodium bicarbonate (NaHCO3) as the stronger the acid‚ the more soluble it is in sodium bicarbonate. b. CH3CH2OCH2CH3 and CH3CH2OH The best solvent to use to differentiate diethyl
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Apparatus 4 test tubes Test tube rack Graduated cylinder (10 mL) 150 mL beaker 250 mL beakers (2) Hot plate Thermometer Safety glasses Beaker tongs Test tube holder Reagents Methanol Methyl-2-propanol 1-pentanol 1-octanol Acetic acid Formic acid (methanoic acid) Salicylic acid Concentrated sulfuric acid (H2SO4) Procedure 1. We labeled the four test tubes A to D and placed them in the test tube rack. 2. Into the appropriate test tubes‚ we poured the correct amount
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Barry Allahyar Dr. Dodd CHEM 2122 2010-09-16 Experiment 19: Fischer Esterification‚ Conclusion The objective in this experiment was to efficiently perform an Fischer esterification of 1-butanol and acetic acid to form water and n-butyl acetate‚ and to confirm the esterification using IR spectroscopy analysis. It was found that 0.734 grams of n-butyl acetate was formed with a percent yield of 61%. The product was confirmed using IR spectroscopy and boiling point confirmation. The reaction mechanism
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Banana Oil Introduction: In this lab the synthesis‚ purification‚ and characterization of isoamyl acetate‚ or banana oil‚ was determined. The synthesis was completed by a reversible esterification reaction which required the heating of glacial acetic acid and isoamyl alcohol‚ combined with a sulfuric acid catalyst in hexane. In order to increase the efficiency of the reaction‚ LeChatelier’s Principle is utilized by removing water from the products. As a result‚ the reaction as a whole shifts the
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Hour Emergency Telephone: Customer Service: Product Disposal Information: CHEMTREC: (989) 496-5900 (989) 496-6000 (989) 496-6315 (800) 424-9300 MSDS No.: 01890573 Generic Description: Physical Form: Color: Odor: Silicone elastomer Paste Colorless Acetic acid odor 2 Flammability Revision Date: 2006/01/23 NFPA Profile: Health Note: NFPA = National Fire Protection Association 1 Instability/Reactivity 0 2. OSHA HAZARDOUS COMPONENTS CAS Number 17689-77-9 4253-34-3 Wt % 1.0 - 5.0 1.0 -
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