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A student followed the procedure of this experiment to determine the percent NaOCl in a commercial...

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Chemistry

A student followed the procedure of this experiment to determinethe percent NaOCl in a commercial bleaching solution that was foundin the basement of an abandoned house. The student diluted 50.00 mLof commercial bleaching solution to 250 mL in a volumetric flask,and titrated a 20-mL aliquot of the diluted bleaching solution. Thetitration required 35.46 mL of 0.1052M Na2S2O3 solution. A fadedprice label on the gallon bottle read $0.79. The density of thebleaching solution was 1.10 g/mL

Calculate the mass of NaOCl present in the diluted bleachingsolution titrated

Answer & Explanation Solved by verified expert
4.4 Ratings (664 Votes)
first Calculate the number of moles of S2O32 ion required for the titration The titration required 3546 mL of 01052M Na2S2O3 solution volume 3546 ml 003546 L    See Answer
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