References 1.) Lehman‚ John. Operational Organic Chemistry‚ 3rd Edition. Experiment 4 (pp. 38-45; 680-687; 644-650)‚ Prentice-Hall‚ 1999. 2.) Laboratory Reference Manual: Experiment 3. Retrieved from: http://academic.reed.edu/chemistry/alan/201_202/lab_manual/expt_salicylic_acid/background.html 3.) Lab 5: Synthesis of Salicylic Acid. Retrieved from: http://academic.evergreen.edu/curricular/whatscookin/Lab%20five%20%20methyl%20saliclate.htm 4.) Handout: Synthesis of Salicylic Acid. Retrieved
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string to a 50 g weight hanger and drape the string over the pulley. The string length should be such that‚ when one hanger hits the floor‚ the upper part of the other hanger is near the pulley‚ without touching the pulley. (You may find that the lab assistant has already set up the apparatus as described here. If so‚ double check the setup.) 2. Place equal masses of approximately 1000 g on each weight hanger. These masses should include four 5 g masses at the top of the left hanger. Hold back
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soil from the site and then take several other samples from different points on the site. This ensures variety of soil to ensure that all the site is safe‚ not just a small area where you would have taken your first sample from. I will return to the lab with the samples of soil I have extracted from the site. Here I will make a solution from the samples in order to carry out the identification tests. In order to turn my soil samples
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Acetic acid MSDS. 2012. “Material Safety Data Sheet Acetic acid MSDS.” Accessed September 3‚ http://www.sciencelab.com/msds.php?msdsId=9922769 Chemlab. 1997-2000. “Chemlab-glassware-burets.” Darmouth College. Sienko‚ Michell and Robert Plane. 1957. Chemistry. McGraw-Hill Book Company‚ Inc.
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Experiment 2 and 3: Synthesis of Aspirin and Determination of Melting Point A. Abstract Aspirin is the common name for the compound acetylsalicylic acid‚ widely used as a fever reducer and as a pain killer. The first part of the experiment aims to synthesize aspirin from the reaction of salicylic acid with acetic anhydride with the aid of phosphoric acid as a catalyst. The second part of the experiment aims to assess the purity of aspirin through the determination of its melting point and
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EXERCISE 11 SYNTHESIS OF ASPIRIN MARAVILLA‚ Ana Mikaela B Group 4 CHEM 40.1 1L Date performed: September 30‚ 2013 Date submitted: October 7‚ 2013 VI. RESULTS AND DISCUSSION Aspirin is prepared by the esterification of salicylic acid with acetic anhydride under acidic conditions. The phenol group in salicylic acid is replaced by a carboxyl group through electrophilic substitution. The mechanism for the reaction can be summarized
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Soluble aspirin tablets Adult dosage: To treat pain or fever in adults‚ the recommended dose is 325 mg to 650 mg every 4 to 6 hours as needed. The maximum daily dose is 4‚000 mg‚ unless otherwise directed by your doctor. For adults with conditions caused by inflammation such as rheumatoid arthritis‚the usual dose is 975 mg 4 to 6 times daily on a regular basis. Sometimes‚ higher doses may be used. To treat migraine headache pain‚ the recommended adult dose is 1‚000 mg at the onset of pain or
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objective was to convert a specific amount of salicylic acid into the same amount of aspirin that was high in purity. Furthermore‚ the other objectives were to enable students to conduct the synthesis of aspirin‚ reinforce skills or recrystallisation and the technique of melting point determination. The amount of each compound should be the same because there is a 1:1 ratio between them. The purity of the synthesized aspirin was measured by determining its melting point and percent yield. Soluble impurities
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Once the aspirin is prepared‚ it is isolated from the reaction solution and then it is purified. The aspirin is insoluble in cold water‚ and it is isolated by filtering the chilled reaction solution. Purification is essential to remove any unreacted salicylic acid and acetic anhydride as well as the acetic acid product and phosphoric acid. Acetic anhydride is caused to decompose by the addition of water once the formation of aspirin is complete. C4H6O3 (Acetic anhydride) + H2O (Water) ------------------------->
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assignment‚ you will dissolve a sample of NaCl in water and then measure the boiling point elevation for the solution. 1. Start Virtual ChemLab and select Boiling Point Elevation from the list of assignments. The lab will open in the Calorimetry laboratory with a calorimeter on the lab bench and a sample of sodium chloride (NaCl) on the balance. 2. Record the mass of the sodium chloride in the data table. If it is too small to read‚ click on the Balance area to zoom in‚ record the reading
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