Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2 with Student Solutions Manual eBook, 4 terms (24 months) Printed Access Card

11th Edition

ISBN: 9781337128469

Author: Darrell Ebbing, Steven D. Gammon

Publisher: Cengage Learning

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Chapter 21, Problem 21.189QP

The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine, because the reaction goes to completion. The amount of iodine produced is then determined by titration with sodium thiosulfate, Na₂S₂O₃, which is oxidized to sodium tetrathionate, Na₂S₄O₆. Potassium iodide was added in excess to 5.00 mL of bleach (density = 1.00 g/mL). This solution, containing the iodine released in the reaction, was titrated with 0.100 M Na₂S₂O₃. If 34.6 mL of sodium thiosulfate was required to reach the endpoint (detected by disappearance of the blue color of the starch iodine complex), what was the mass percentage of NaClO in the bleach?

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Chapter 21, Problem 21.188QP

Chapter 21, Problem 21.190QP

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Chapter 21 Solutions

Bundle: General Chemistry, Loose-leaf Version, 11th + OWLv2 with Student Solutions Manual eBook, 4 terms (24 months) Printed Access Card

Ch. 21.9 - Considering the fact that N2 makes up about 80% of...Ch. 21.10 - Prob. 21.2CC Ch. 21 - Prob. 21.1QP Ch. 21 - Prob. 21.2QP Ch. 21 - Prob. 21.3QP Ch. 21 - Prob. 21.4QP Ch. 21 - Prob. 21.5QP Ch. 21 - Prob. 21.6QP Ch. 21 - Prob. 21.7QP Ch. 21 - Prob. 21.8QP

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Solution Summary: The author explains how the mass percentage of NaClO can be calculated by taking the calculated mass to the total mass of the sample whole multiplied by 100.

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