Experiment 12: Isopentyl Acetate 19 October 2012 Introduction: The purpose of this experiment is to prepare isopentyl acetate by direct esterification of acetic acid with isopentyl alcohol. After refluxing there is an isolation procedure where excess acetic acid and remaining isopentyl alcohol are easily removed by extraction with sodium bicarbonate and water. The ester is then purified by simple distillation and the IR is then obtained. Techniques and equipment used throughout the experiment
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formed from octanol (octyl alcohol) and acetic acid. It is mostly found in oranges and other citrus products. Octyl acetate can be synthesized by a condensation reaction: C8H17OH + CH3COOH → C10H20O2 + H2O Uses Because of its fruity odor‚ octyl acetate is used as the basis for artificial flavors and in perfumery. It is also as a solvent for nitrocellulose‚ waxes‚ oils and some resins. Source: http://en.wikipedia.org/wiki/Octyl_acetate Acetic Acid Acetic acid /əˈsiːtɨk/ (systematically named ethanoic
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the banana oil lab we began with isopentyl alcohol + acetic acid isopentyl acetate + Water. We needed for this experiment a hot plate‚ clamps‚ pipette‚ 5mL vial‚ caps‚ hoses and a thermometer. Upon starting‚ our group set up an open system experiment that allowed gases to be released to avoid pressure build up. We mixed together to molecules‚ 1.0mL of isopentyl alcohol‚ 1.5mL of acetic acid and added three drops of sulphuric acid. The acetic acid was used as a catalyst to speed up the reaction
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showing the reaction that takes place between zinc and iodine using only deionized water instead of acetic acid (or vinegar) as we did in the previous lab by adding acetic acid to zinc iodide. The purpose of this lab was to see how water created the reaction and another compound or precipitate. Focus Question: Zn(OH)2 was the product when zinc and iodine were reacted without the presence of acetic acid in the water. Confidence Report: I am confident that our data in the experiment was “good data”
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current experiment was to determine the pH of various hydrochloric acid and acetic acid solutions‚ to determine the pH of various salt solutions‚ to prepare a buffer solution‚ and determine the effects of adding a strong acid and strong base to the buffer solution versus adding a strong acid and strong base to water. The measured pHs for the hydrochloric acid solutions were 1.6‚ 2.2‚ 2.9‚ and 3.8. The measured pHs for the acetic acid solutions were 2.9‚ 3.9‚ 4.2‚ and 4.4. The pHs measured for the salts
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to see how given amounts of sodium bicarbonate reacts with acetic acid and see how it creates different amounts of new compounds. Procedure: In this lab‚ we were going to be reacting 12.5g sodium bicarbonate with 7.4mL acetic acid. Before we began‚ we turned on the hot plate to a medium level‚ allowing it time to heat up. While the plate was heating‚ we gathered 1 1/4g sodium bicarbonate onto the balance. Next‚ we measured 7.4mL acetic acid by pouring it into a 10mL graduated cylinder. Once we
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smell of esters Method Place 250 mL of deionized water in a 500 mL. Heat this water until it boils. Turn off the heat source after boiling Follow the chart below for the following steps Ester # Acid Alcohol 1 Acetic Acid Butanol 2 Acetic Acid Octanol 3 Acetic Acid Methanol 4 Acetic Acid Ethanol 5 Butanoic acid Butanol 6 Butanoic acid Octanol 7 Butanoic acid Methanol 8 Butanoic acid Ethanol Place tens drops of the acid in your test tube. Add 10 drops of the required alcohol
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Analyze energy sources and transfers of heat. 3.8.10A Analyze the relationship between societal demands and scientific and technological enterprises. Content Objectives Students will know that 1. Acetic acid reacts with sodium bicarbonate to produce a gas. 2. Acetic acid and sodium bicarbonate are the chemical names for vinegar and baking soda‚ respectively. 3. The two main purposes of an air bag are to slow a person’s forward movement into the steering wheel (or dashboard)
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weighing boats and an electronic scale. We poured the NaHCO3 from the plastic weighing boats into their own plastic bags. Using the measurements of the NaHCO3 ‚ we calculated the exact volumes of 6.0 M acetic acid needed to completely react with the amounts of NaHCO3 (see Calculations). The acetic acid was then measured out using 10 mL graduated cylinders and poured into their respective locations in the plastic bags. Once all of the reactants were placed into their correct positions‚ the bags were
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Solubility 1. Prepare 3 test tubes with 3 ml of water in each. 2. Place 3 drops of acetic acid‚ benzoic acid‚ and oxalic acid in separate test tubes. 3. Shake and observe the solubility‚ then test the solution with litmus paper if soluble. 4. Repeat the experiment using ether and ethanol as the solvent. 9.2 Reactions with Bases 1. Prepare 3 test tubes with 3 drops of 5% NaOH. 2. Add 5 drops of 50 mg of acetic acid‚ benzoic acid and oxalic acid. 3. Shake and observe the changes. 4. Repeat
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