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A 3.00-mL bleach (NaOCl is the active ingredient) sample is mixed with potassium iodide and acid to completely form triiodide (I3 - ) ions. You then titrate the I3 − ions with a thiosulfate (S2O3 2− )...

A 3.00-mL bleach (NaOCl is the active ingredient) sample is mixed with potassium iodide and acid to completely form triiodide (I3 - ) ions. You then titrate the I3 − ions with a thiosulfate (S2O3 2− ) solution you have previously determined to be 0.1306 M. The endpoint is reached when 31.52 mL of the thiosulfate solution is added. What is the molar concentration of the bleach solution? What is its mass percent?

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The threa veachons that takes place ave Hypochlorous aud (an) 3 thiosulPhate Fyom the alove euations, it is clea that 2. o 13o. 130 6 x 31 52 vw 2 о. 1306x 31,52 mmRNaod 2 2 Mass of 31 S2 130 6 3S.5 2. MASS of NAO c 2. o. 15 33g Nos MaSS 2 3-33 3- 33Sleach Soluhon o 1306 x 31-52 mmof Naod Cal aulated a beve 2. Given volume of 8leach - Molav Concen tation o. 130 6x 31 S2 mm

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A 3.00-mL bleach (NaOCl is the active ingredient) sample is mixed with potassium iodide and acid to completely form triiodide (I3 - ) ions. You then titrate the I3 − ions with a thiosulfate (S2O3 2− )...
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