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Redox Titration - molarity of our standard thiosulfate to...

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Redox Titration: Analysis of Bleaches March 29, 2008 Introduction In this lab, we used oxidation-reduction reactions as an analytical tool. We diluted a solution of sodium thiosulfate and titrated it into a solution of 0.010 M potassium iodate, 10% KI and 1.0 M sulfuric acid. We then found the concentration of sodium hypochlorite, the oxidizing agent. Chemical Responsibility We worked with hazardous substances in this lab. Sodium thiosulfate is slightly toxic by ingestion and a body tissue irritant. Potassium iodate is an oxidizer, moderately toxic and a tissue irritant. Sulfuric acid is corrosive and can cause skin burns. Commercial bleach is a corrosive liquid, causes skin burns and is moderately toxic by ingestion and inhalation. In addition, commercial liquid bleaches containing sodium hypochlorite are corrosive to the skin and eyes. Sample Calculations Results We titrated the sodium thiosulfate three times, yielding the average
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Unformatted text preview: molarity of our standard thiosulfate to be .0855 M. This calculation was found from the stoichiometry and the volumes used in the experiment. This indicates that the sodium thiosulfate is slightly more dilute than it should have been (around .1 M). Due to this inaccuracy, the calculated percentage of sodium hypochlorite was probably lower than it should have been. We calculated it to be 5.34%. Household bleach claimed to be 6% sodium hypochlorite, so our results were still close. Post Lab Questions (attached) Conclusion Oxidation-reduction reactions can be used to determine various things about solutions. In this lab, we used it to determine the percentage of hypochlorite ion in laundry bleaching solutions. We were able to calculate this by using the same methods as you would for an acid-base reaction, and applying information we know about the mass, volume and concentrations....
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