10.00 mL of aqueous NaOCl is treated with excess potassium iodide, KCl, in an acidicsolution. The iodine that gets formed is completely titrated with 35.50 mL of 0.0250 MNa2S2O3 solution, evident by the complete disappearance of the dark-blue color of theiodine-starch complex.What is the molarity of the NaOCl solution?
10.00 mL of aqueous NaOCl is treated with excess potassium iodide, KCl, in an acidicsolution. The iodine that gets formed is completely titrated with 35.50 mL of 0.0250 MNa2S2O3 solution, evident by the complete disappearance of the dark-blue color of theiodine-starch complex.What is the molarity of the NaOCl solution?
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter21: The Chemistry Of The Main Group Elements
Section21.5: The Alkaline Earth Elements, Group 2a
Problem 1Q
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10.00 mL of aqueous NaOCl is treated with excess potassium iodide, KCl, in an acidic
solution. The iodine that gets formed is completely titrated with 35.50 mL of 0.0250 M
Na2S2O3 solution, evident by the complete disappearance of the dark-blue color of the
iodine-starch complex.
What is the molarity of the NaOCl solution?
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