f. Calculate the mass of commercial bleaching solution titrated.g. Determine the percent NaOCl in the commercial bleaching solution.h. Calculate the mass of one gallon of the commercial bleaching solution.i. Calculate the cost of 100 g of the commercial bleaching solution.j. Determine the cost of the amount of commercial bleaching solution required to supply 100 g of NaOCl. 38 General Chemistry Laboratory Investigations. Volume 2 Duquesne University3. A student followed the procedure of this experiment to determine the percent NaOCI in a commercialbleaching solution that was found in the basement of an abandoned house. The student diluted50.00 mL of the commercial bleaching solution to 250 mL in a volumetric flask, and titrated a 20-mLaliquot of the diluted bleaching solution. The titration required 35.46 mL of 0.1052M Na2S₂O3 solution. Afaded price label on the gallon bottle read $0.79. The density of the bleaching solution was 1.10 g mL-¹.a. Calculate the number of moles of S₂O32- ion required for the titration.b. Calculate the number of moles of 12 produced in the titration mixture.c. Calculate the number of moles of OCI" ion present in the diluted bleaching solution titrated.d. Calculate the mass of NaOCl present in the diluted bleaching solution titrated.e. Determine the volume of commercial bleaching solution present in the diluted bleaching solutiontitrated.

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Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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f. Calculate the mass of commercial bleaching solution titrated. g. Determine the percent NaOCl in the commercial bleaching solution. h. Calculate the mass of one gallon of the commercial bleaching solution. i. Calculate the cost of 100 g of the commercial bleaching solution. j. Determine the cost of the amount of commercial bleaching solution required to supply 100 g of NaOCl.

38 General Chemistry Laboratory Investigations. Volume 2 Duquesne University
3. A student followed the procedure of this experiment to determine the percent NaOCI in a commercial
bleaching solution that was found in the basement of an abandoned house. The student diluted
50.00 mL of the commercial bleaching solution to 250 mL in a volumetric flask, and titrated a 20-mL
aliquot of the diluted bleaching solution. The titration required 35.46 mL of 0.1052M Na2S₂O3 solution. A
faded price label on the gallon bottle read $0.79. The density of the bleaching solution was 1.10 g mL-¹.
a. Calculate the number of moles of S₂O32- ion required for the titration.
b. Calculate the number of moles of 12 produced in the titration mixture.
c. Calculate the number of moles of OCI" ion present in the diluted bleaching solution titrated.
d. Calculate the mass of NaOCl present in the diluted bleaching solution titrated.
e. Determine the volume of commercial bleaching solution present in the diluted bleaching solution
titrated.

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