The following method is reported in Standard Methods for the Examination of Water and Wastewater for...
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The following method is reported in Standard Methods for the Examination of Water and Wastewater for the analysis of sodium hypochlorite (NaOCI) in bleach. . a 20.00 mL sample of bleach is diluted to 100.0 mL. • a 25.00 mL aliquot of the diluted sample is then transferred into a flask and treated with an excess acidic iodide solution. • the iodine thus formed, is titrated with a standard thiosulfate solution. The chemistry is outlined below (unbalanced equations): Excess iodide is reacted with the analyte in an acidic solution. OCT + I + H → CI+ 1₂ + H₂O The resulting iodine (1₂) is then titrated with a standardized solution of sodium thiosulfate. S₂O3 + 1₂ → S40² + I If 12.62 mL of a 0.00400 N thiosulfate solution was required to reach the end point, what is the concentration of the original bleach solution as wt% and ppm as Cl₂? The following method is reported in Standard Methods for the Examination of Water and Wastewater for the analysis of sodium hypochlorite (NaOCI) in bleach. . a 20.00 mL sample of bleach is diluted to 100.0 mL. • a 25.00 mL aliquot of the diluted sample is then transferred into a flask and treated with an excess acidic iodide solution. • the iodine thus formed, is titrated with a standard thiosulfate solution. The chemistry is outlined below (unbalanced equations): Excess iodide is reacted with the analyte in an acidic solution. OCT + I + H → CI+ 1₂ + H₂O The resulting iodine (1₂) is then titrated with a standardized solution of sodium thiosulfate. S₂O3 + 1₂ → S40² + I If 12.62 mL of a 0.00400 N thiosulfate solution was required to reach the end point, what is the concentration of the original bleach solution as wt% and ppm as Cl₂?
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