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
