Analysis of two Commercial Brands of Bleaching Solution Essay

ObjectiveTo determine the concentrations of the active ingredients in 2 commercial bleaches.IntroductionSodium hypochlorite is usually found in bleaching answers. It is the active ingredient of bleaching solutions. It bleaches by oxidation. When it is added to dye, the following reaction occursClO- + dye - Cl- + (dye + O)If the oxidized form of the dye is colorless, then the color of the dye would fade away.In the front man of acid, the hypochlorite ions from the bleaching solution reacts with the iodine ions from potassium iodide in the following wayClO- + 2I- + 2H+ I2 + H2O + Cl-When atomic number 11 thiosulphate solution is added into this reacted solution, a further reaction occursI2 + 2S2O32- 2I- + S4O62-This reaction could be employ in titration to find out the number of moles of thiosulphate ions, thus the concentration of hypochlorite ions in the bleaching solution.Procedure1. 10 cm3 of Kao Bleach was pipette into a volumetric flask. Distilled water was added until the me niscus reaches the graduation point.2. 25 cm3 of the titrated bleach was pipette into a conical flask. About 10 cm3 of potassium iodide and dilute sulphuric acid was added into the conical flask.3. The solution was titrated with sodium thiosulphate solution until the brown colour of the iodine fades.4. Starch solution was added into the conical flask, and the solution was further titrated until the dark-brown colour of the starch-iodine complex turns to colourless. The volume of sodium thiosulphate solution required to reach the end point was recorded.5. Steps 1 to 4 were repeated 3 more times.6. Steps 1 to 5 were repeated apply Clorox Bleach.Data and CalculationMolarity of standard Na2S2O3 solution = 0.05182MBrand A KaoPrice $11.9/ 1500mlTrial123Final reading/cm326.823.125.726.0 sign reading/ cm34.10.42.93.2Volume of Na2S2O322.722.722.822.8