The Mass of Acetylsalicylic Acid in Aspirin ------------------------------------------------- Purpose The purpose of the lab is to determine the mass of the ‘active ingredient’ in a commercial ASA tablet. ------------------------------------------------- ------------------------------------------------- Introduction There are three main theories surrounding acids and bases including the Arrhenius‚ Bronsted-Lowry‚ and Lewis theories. The Arrhenius theory of acids and bases states that
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BACKGROUND: Esterification is a reaction that combines an alcohol with an organic acid‚ with a water molecule is being taken out‚ and an ester is formed. A concentrated acid catalyst speeds up the esterification. In this experiment set up‚ sulphamic acid was used‚ as it is a solid acid and be added dry‚ without any water‚ which is a reactant in this experiment equilibrium. Esterification is a slow and reversible reaction. The equation for the reaction between an acid RCOOH and an alcohol RẬᶦ
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220_002 #04 FOOD & BEVERAGE A P P L I C AT I O N N O T E Page : 1 CARBOHYDRATES IN FOOD THE FINEST LC-EC APPLICATIONS FOR FOOD & BEVERAGE ANALYSIS EVER PROCESSED INTRODUCTION Carbohydrates not only provide the most easily accessible energy source for our body‚ they also play an important role in many physiological processes. They are involved in intercellular recognition‚ infection processes‚ and certain types of cancer. Carbohydrates analysis is of interest to the food industry but
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Name: ____________________________________ Locker Number: ____________________________ CHEMISTRY 354-355 Experiment 2 SOLUBILITY 1. Part A. Solubility of Solid Compounds. Use your observations to complete the following table‚ rating each system as soluble‚ insoluble‚ or partially soluble. Organic Compound Benzophenone Water Methyl Alcohol Hexane Malonic acid Biphenyl 2. Considering the polarities of the compound and the solvent and the potential for hydrogen bonding‚ answer the
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range. Each group (I was with William Yung for this experiment) was tasked with testing one homogenate. The homogenate tested by our group was liquid spinach. Each team added HCl and NaOH to their homogenate. As we found out in our experiment‚ HCl was an acid so when added to the liquid spinach the pH lowered and NaOH‚ being a base‚ rose the pH level when added. The better the buffer the homogenate is‚ the less its pH changes
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experimentation. We tested the solubility of each of the starting and ending materials in water‚ HCl‚ NaOH‚ toluene‚ and acetone. We discovered that the starting materials would only dissolve in toluene. To make the soap‚ we obtained about 10 mL of vegetable oil and 10 g of lard and we placed them both in separate 250 mL beakers. While we were stirring the compounds‚ we also added 15 mL of 6 M NaOH drop by drop and 1 mL of glycerol. We then heated our solutions to boiling on a hot plate. Once the
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Discovering the Mystery of Eleven Test Tubes Karen Radakovich Ph.D. Mohammad Farhad Brittany Cina CH 223‚ Spring 08 Abstract: Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4‚ 6M NH3‚ 6M HCl‚ 6M NaOH‚ 1M NaCl‚ 1M Fe(NO3)3‚ 1M NiSO4‚ 1M AgNO3‚ 1M KSCN‚ 1M Ba(NO3)2‚ 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9‚ ammonia which was identified by its pungent odor
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The first test performed was the Metal Hydroxide Test‚ wherein drops of 6 M NaOH were added dropwise to each tube until a precipitate was formed‚ or a total of 20 drops were administered. This process was repeated for each tube‚ with drops administered until a precipitate was visible. Drops were administered as follows:K+: 20 drops‚ Zn2+: 3 drops‚ Cu2+: 2 drops‚ Co2+: 2 drops 6 M NaOH added. The results were recorded following each cation‚ noting the color
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To hold the solution and mix the indicator and NAOH Burette To let me pour the HCL into the conical flask at a continuous rate Boss clamp To hold the burette Pipette sucker To pull up the chemicals Beakers To hold the chemicals into so they won’t spill Pipette To accurately measure out the 25 cm3 Measuring cylinder To accurately measure out the chemicals 50 cm3 of HCL To use in the experiment to see the concentrations 50 cm3 of NAOH To use in the experiment to see the concentrations
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between sucrose and water. 2. For solutes that are dissolved because of reaction with the solvent‚ write the balanced equation involved. Balanced Equation A C6H5OH + NaOH C6H5ONa + H2O D C6H5CHO + H2SO4 m-benzaldehyde sulfonic acid E C6H5CH2OH + H2SO4 C6H5CH2OH2+ + HSO4- G C6H5COOH + NaOH C6H5COONa + H2O C6H5COOH + NaHCO3 C6H5COONa + CO2 + H2O H C6H5NH2 + HCl → C6H5N+H3Cl- 3. On the basis of solubility behaviour‚ determine the best solvent to differentiate
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