Equipment Materials
50.00 ml buret, 250.ml volumetric flask, 1.00 ml volumetric pipet 10.0 mL volumetric pipet, 25.00 mL volumetric pipet, pipettor, 250 mL Erlenmeyer flask, 10.0 mL graduated cylinder, several beakers, several watchglasses, unkown bleach solution, 10% potassium iodide solution, 2M hydrochloric acid solution, 0.150 M sodium thiosulfate solution, 1% starch solution.
Background information regarding this experiment is as follows:
An aqueous solution of sodium hypochlorite (NaOCI) is a clear, slightly yellow liquid, and is commonly known as bleach. Aside from its uses as a bleaching agent, sodium hypochlorite solutions are also used as sterlizing agents and in water treatment. Industrial uses include agricultural, food handling, paper production, and textile production. Sodium hypochlorite is also added to waste water to reduce odors.
The concentration of sodium hypochlorite in bleach solutions can be determined by titration. Therefore, we must use a two-step method to titrate sodium hypochlorite. In the first step, sodium hypochlortie, hydrochloric acid, iodide ion, and starch are combined to form a starch-triiodide complex. In this step there are 3 reactions that take place:
The result of these 3 reactions is that when sodium hypochlorite is present the starch-triiodide complex is produced.
In the second step the starch-triiodide product is titrated by sodium thiosulfate to form a colorless solution of iodide, dithionate.
I do not know how to answer the following on the data sheet: (? means I do not know how to answer)
Table 1:
Mass of 1.00 ml of unknown (by tare): 10.552 g
Density of bleach: (g/ml) : 1.055 g/ml
Volume of diluted bleach used in each titration: 10.00
Concentration of sodium thiosulfate: ? (M)
Titration Data:
Initial buret reading (ml): trial1: 0.000 ml Trial 2: 0.00 ml Trial 3: 0.000ml
Final buret reading (ml): trial 1: 13.50ml Trial 2: 13.30ml Trial 3: 13.40ml
Volume delivered(ml: trial 1: ? Trial 2: ? trial 3:?
Calculations: (show clearly)
For trial 1,2,3 ???
1.Moles of Na2S2O3 in titration: ??? trial 1,2,3
2.Moles of NaOCl: ???trial 1, 2,3
3.Average moles of diluted NaOCl: (one answer) ?
4.Average moles of undiluted NaOCl: (one answer.. mol) ?
5.Standard Deviation: (one answer) (mol)
6.Average mass of NaOCl in 25.00mL of undiluted bleach: ? (g)
7.mass of 25.00 mL of undiluted bleach: ? (g)
8. Mass % of NaOCL from experiment: ? (%)
9.Actual mass % of NaOCL (from prof; student does not make an entry):? (%)
More questions all need to be answered please:
1. Calculate the volume of the reagent thiosulafte solution which would be required if you titrated a 25ml sample of the original commercial bleach instead of 25ml of the diluted solution.
2. Why would we choose a graduated cylinder to measure the HCl and KI solutions instead of a volumetric pipette? When would we use a volumetric pippette?
3. You calculated the mass percent of sodium hypochlorite in the bleach( dilute and undiluted). Now calculate the molarity of the sodium hypochlorite in the diulte and undiluted solution/
4. Use oxidation states to show that equations (2) and (4) in the introduction are redox reactions and that equation 1 is not a redox reaction. :
-(1) NaOCl(aq) + HCl(aq) yields HOCl(aq)+NaCl(aq)
-(2) HOCL (aq) + HCl(aq) + 3I(aq) yields I3(aq) + 2CL(aq) + H2O(l)
-(4) (I3) (Starch) + 2S2O3 yields 3I + S4O6 + starch
5. combine equation 1-3 to show the overall reaction for the products of the starch-triiodide complex.
-(1) NaOCl(aq) + HCl(aq) yields HOCl(aq)+NaCl(aq)
-(2) HOCL (aq) + HCl(aq) + 3I(aq) yields I3(aq) + 2CL(aq) + H2O(l)
-(3) I3 + Starch yields (I3) (Starch)
6. What standard was used in this experiment?
7. Describe the naming of NaClO and HClO. What are the names of the following compounds? NaClO2 , NaClO3, NaClO4 , HClO2, HClO3, HClO4
8 Submit a one paged (typed double spaced) report that discusses the following topics:
a. the goals or objectives of the experiment
b.your results as they relate to the goals and objectives
c. the quality of your results.
