are bleaches‚ hair coloring agents‚ scouring powders‚ and toilet bowl cleaners. The most common oxidizing agent in bleaches is sodium hypochlorite‚ NaClO (sometimes written NaOCl). Commercial bleaches are created by bubbling chlorine gas into a sodium hydroxide solution (remember this from your “funky redox rxns”?). Some of the chlorine is oxidized to the hypochlorite ion‚ ClO- and some is reduced to the chloride ion‚ Cl- (a disproportionation reaction). The solution remains strongly basic. The
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! ! To review oxidation-reduction reactions and their stoichiometry. To learn the concept and technique of redox titration. To determine the percent (m/v) of an active ingredient‚ sodium hypochlorite (NaOCl)‚ in a commercial bleaching agent. B. Theoretical Background Whereas acid-base reactions involve the transfer of a proton‚ oxidation-reduction or redox reactions involve the transfer of electrons from one substance to another‚ resulting in changes in oxidation numbers of two or more
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manipulation of a molecule‚ be it in oxidation‚ reduction‚ or in the addition of a functional group. In this lab we will examine the stereoselectivity of the reduction of 4-tert-butylcyclohexanone (Figure 1) using sodium borohydride (Figure 2). In the first week of this lab we will use sodium hypochlorite (Figure 3) to oxidize (Mechanism: Figure 6) commercial 4-tert-butylcyclohexanol‚ synthesizing 4-tert-butylcyclohexanone and using IR analysis to confirm that our oxidation was successful. In the second
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perform a redox titration. To determine the amount of hypochlorite ion present in commercial bleach. Introduction Many commercial products‚ such as bleaches and hair coloring agents‚ contain oxidizing agents. The most common oxidizing agent in bleaches is sodium hypochlorite‚ NaClO (sometimes written NaOCl). Commercial bleaches are made by bubbling chlorine gas into a sodium hydroxide solution. Some of the chlorine is oxidized to the hypochlorite ion‚ ClO-‚ and some is reduced to the chloride ion
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COMPOUND – Sodium Hypochlorite * Page 12 : The Basics * Page 13 : Chemical Properties * Page 14 : Physical Properties * Page 15 : Safety Precautions * Page 16 : What else is it used in? * Page 17 : References Household Chemical: Bleach Product Use This product is used for: * Removing Stains * Whitening Whites * Killing Germs Chemical Ingredients * Water * Sodium hypochlorite * Sodium chloride * Sodium carbonate * Sodium hydroxide * Sodium polyacrylate
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Analysis of Commercial Bleach Lab I. Purpose In this experiment‚ the amount of sodium hypochlorite in a commercial bleach will be determined by reacting it with sodium thiosulfate in the presence of iodide ions and starch. A solution of sodium thiosulfate of known concentration will be added to the bleach using a buret in a titration procedure. The disappearance of the dark blue color of the starch-iodine complex will signal the end point. II. Procedures Pre-Lab Questions 1. What is
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was conducted. A change in the strip to a deep blue color would signal an excess of sodium hypochlorite reagent present. An excess is the reagent symbolizes the end of the reaction because there is no longer any reactant left to consume reagent. After the reaction was deemed completed‚ the product was isolated and purified by ether extraction‚ aqueous extraction and evaporation. To determine how sodium hypochlorite acts as an oxidizing agent‚ the starting diol and final product were characterized
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Oxidation of Borneol to Camphor Objectives: The purpose of this experiment was to use oxidation to convert (1S)-(-)-borneol into (1S)-(-)-camphor‚ which was done via the use of reagents such as glacial acetic acid and sodium hypochlorite and laboratory techniques learned in previous labs. Afterward‚ the final desired product was obtained‚ and to characterize and ensure the purity of the product‚ further lab techniques were implemented. Overall Reaction: 0 out of 10 Oxidation Reaction:. Mechanism:
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drops of sodium hypochlorite necessary to make a diluted food dye change to colorless in less than three minutes helps calculate the absorbance which can then be analyzed to find the pseudo rate constant and eventually leading to the rate constant and the rate law. The results show that the m and n are both 1st order which makes the overall order of the blue dye 2nd order. Results: In this experiment‚ rate laws and graphs help calculate the oxidation of food dyes by sodium hypochlorite. During the
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Experiment 8 Unique # 51070 The main purpose of the experiment involves two oxidation-reduction reactions to calculate the oxidizing capacity of a sample of unknown bleach. In order to determine the volume of Na2S2O3 added‚ students will conduct a titration of bleach with thiosulfate with addition of a starch indicator to find the end point of the titration. Moreover‚ the oxidizing capacity of bleach is calculated with the percentage by mass of NaOCl in the unknown bleach sample. The overall
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