the best methods is the iodine-thiosulfate titration procedure. The iodide ion‚ I-‚ is easily oxidized by almost any oxidizing agent. In acid solution‚ hypochlorite ions oxidize iodide ions to form iodine‚ I2. The iodine that forms is then titrated with a standard solution of sodium thiosulfate. The analysis takes place in a series of steps: 1. Acidified iodide ion is added to hypochlorite ion solution and the iodide is oxidized to iodine. 2 H+(aq) + ClO-(aq) + 2 I-(aq)
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To carry this out‚ our method combines sodium iodide and common bleach as the oxidizing agent in aqueous alcohol as the solvent. Balanced Chemical Equations: Physical Properties: Name of Chemical Chemical Structure Molar Mass (g/mol) BP/MP (ºC) Density (g/mL) Mass/Vol. Used Purpose 3-methoxy-4-hydroxybenzaldehye C8H8O3 152.1494 MP=81-83‚ BP=285 NA 0.1g Solute Ethanol CH3CH2OH 46.0688 MP=-114.1‚ BP=78.3 0.789 2.0mL Solvent Sodium Iodide NaI 149.8943 MP=661‚ BP=1300 3.667 0.117g Catalyst
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Discussion and Conclusion: Preparation of 1-Bromobutane The purpose of this experiment was to demonstrate the conversion of a primary alcohol‚ 1-butanol‚ to a primary bromoalkane‚ 1-bromobutane‚ a SN2 reaction. The conversion of 1-butanol to 1-bromobutane relies on sulfuric acid which plays two important roles. First‚ it protonates the alcohol of 1-butanol to form an oxonium ion which is a good leaving group. Secondly‚ it produces the hydrobromic acid‚ the nucleophile‚ which attacks 1-butanol
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(NaOCl)‚ is determined by redox titration. The method used is iodine-thiosulfate titration. It is a very useful method‚ since the iodide ion‚ I-‚ is easily oxidized by almost any oxidizing agent. The analysis takes place in a series of steps as follows: 1. A diluted sample of the bleach will be allowed to react with potassium iodide in acidic solution. The iodide ion will be oxidized to iodine while the hypochlorite ion will be reduced to chloride (Equation 1). 2 H+(aq) + OCl-(aq) + 2 I-(aq)
Free Oxidizing agent Sodium Iodine
Phenyl Salicylate per parts A‚ B‚ C * 2 g Potassium Iodide per parts A‚ B‚ C * 2 g Sodium Chloride per parts A‚ B‚ C * 2 g Sucrose per parts A‚ B‚ C * 6 Bunsen Burners * 6 Test Tubes with 25 ml Ethanol each * 6 Test Tubes with 25 ml Water each * 6 100 ml beakers with 50 ml Water each * 10 g Calcium Chloride per parts D * 10 g Citric Acid per parts D * 10 g Phenyl Salicylate per parts D * 10 g Potassium Iodide per parts D * 10 g Sodium Chloride per parts D
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Using the Iodine clock method to find the order of a reaction Introduction When peroxodisulfate (VI) ions and iodide ions react together in solution they form sulfate (VI) ions and iodide. This reaction is shown below: S2O82-aq+ 2I-aq SO42-aq+ I2(aq) The reactants and the sulfate (VI) ions are colourless however the Iodine is a yellow/brown colour. This allows you to measure the progress of the reaction through the colour change when the iodine is produced. In order to determine the order of
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Cloud seeding can be performed from the ground using a launcher with silver iodide cartridges‚ that get shot into the clouds. Or the process can be done from an aeroplane that releases the silver iodide into the clouds from above. Using aeroplanes is the preferred method as it is more accurate. Ground Based Cloud Seeding is used in places where there is low level clouds over difficult terrain
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EXPERIMENT 4 TITLE Complex Formation and Precipitation. INTRODUCTION Precipitation is the formation of a solid in a solution as the result of either a chemical reaction‚ or supersaturating a solution with a salt resulting in solid material collecting on the bottom of the beaker (Housecroft & Constable‚ 2006). When the solution has been supersaturated by a compound and no more material can be supported by the solution‚ it considered as precipitate. Commonly‚ the solid will fall out of the
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acidic medium. However‚ iodine is not very soluble in water (0.001M)‚ this makes the method less than ideal. Instead of dissolving solid iodine in water‚ we can obtain excess quantity of iodine solution by adding an unmeasured excess of potassium iodide solution to a known volume of an acidified standard potassium iodate solution according to the following equation: IO3-(aq) + 5 I- (aq) + 6 H+ (aq) 3I2 (aq) + 3H2O (l) Then the experiment is immediately followed by a back titration of the excess
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importance of the electron in the formation of these new bonds. Materials Boileezers (boiling chips) Desiccant 0.17M acetic acid (acidified water) Solution of Sodium thiosulfate Granular zinc Iodine crystals Zinc ion and iodine-iodide-triiodide ion in water Solid zinc iodide Mineral oil Silver nitrate Magnesium turnings 3M Hydrochloric acid (HCl) solution 2 boiling tubes 1 large tube (we used a small) Pipet Beakers (to hold tubes) Bunsen burner PART 1 Procedure Get a boiling tube and label it R (reactants)
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