redox - manipulations, we calculated the average molarity...

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Redox Titration Introduction - The goal of this week’s experiment was to analyze the percentage of hypochlorite ion in laundry bleaching solutions using redox titration analysis. By measuring the amount of sodium thiosulfate necessary to titrate the solution, we could calculate the percentage of hypochlorite ions. Chemical Responsibility - In this lab, sodium thiosulfate, potassium iodate, sulfuric acid, and commercial bleach are all dangerous compounds and must be handled with care. All solutions are to be disposed of in the proper waste containers labeled at the front of the room. Report Sheet/Sample Calculations- See report sheet. Discussion - For the first trial, we determined the potassium iodate standard by measuring the sodium thiosulfate necessary to titrate the solution. Using some chemical
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Unformatted text preview: manipulations, we calculated the average molarity of Na2S2O3 to be .107M. Using this data, we were able to manipulate the numbers using a number of calculations. The mass of NaOCl present was about .072g and the mass of the bleach was 1.084g. When the latter is divided by the former, you get an average of 6.65% NaOCl present in commercial bleach Conclusion-A major portion of the calculations was based on mole to mole ratios of the reactions. Without an understanding of these, the calculations would have been impossible. Despite having a low percentage of hypochlorite ions, bleach is still very basic, which demonstrates how powerful each hypochlorite ion actually is....
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This note was uploaded on 04/08/2008 for the course CHM U212 taught by Professor Witten during the Spring '08 term at Northeastern.

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