Mass of tablet= 1.104g Initial mass of sample (g)=1.080g Initial volume of burette=50mL (mL) Final volume of burette=40mL (mL) Volume of KIO3 (mL)=10mL Molarity of KIO3 solution = ? (from part 1) Moles of KIO3 Moles of C6H8O6 Mass of C6H8O6 (g
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- Initial volume of burette = 50 mL - Final volume of burette = 40 mL - Volume of KIO3 used = Initial volume - Final volume = 50 mL - 40 mL = 10 mL Show more…
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Part I. Standardization of the Sodium Thiosulfate Solution Molarity of the KIO3 stock solution. 0.0047 Show your calculations. (Hint: You are given the density of KIO3 stock solution.) mass = 122.5 g Density = 1 g/mL V = 0.5840 mL 0.5840 / 122.5 g * 1 g/mL = 0.0047 Complete the following table. Trial 1 Trial 2 Trial 3 Final burette reading (mL) 20.24 20.45 21.51 Initial burette reading (mL) 0.04 0.21 0.96 Volume of Na2S2O3 (mL) 20.2 20.24 20.55 Average volume. 20.33 mL 0 Standard deviation of sample (up to 3 sig. figs.). Average Molarity of the Na2S2O3. Show your calculations.
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Report Sheet Oxidation-Reduction Titrations I: Determination of Oxalate C. Analysis of Oxalate Complex or Unknown Mass of sample Trial 1 Trial 2 Trial 3 Weighing bottle initial mass 3.253 g 3.274 g 3.268 g Weighing bottle final mass 3.373 g 3.394 g 3.388 g Mass of sample .12 g .12 g .12 g Titration Final reading 17.6 ml 17.8 ml 18.4 ml Initial reading .2 ml .2 ml .2 ml Volume of KMnO4 17.4 ml 17.6 ml 18.2 ml Calculations Millimoles of oxalate, C2O4 2- Mass of oxalate, C2O4 2- Percent oxalate, C2O4 2- Average percent oxalate Standard deviation If you analyzed your oxalate complex from earlier, complete the following: Theoretical percent oxalate in your complex (show calculations) Determine the purity of your complex as (experimental % oxalate / theoretical % oxalate) x 100% = % purity.
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Based on the following two reaction equations, calculate the molarity of an unknown ascorbic acid if titrating 15 mL of this unknown solution consumes 15.67 mL of 0.01235 M of KIO3 solution to reach the endpoint. [1] KIO3 + 5KI + 6H+ → 3I2 + 6K+ + 3H2O [2] C6H8O6 + I2 → C6H6O6 + 2I- + 2H+ Hint: Each KIO3 produces 3 molecules of I2, and each I2 molecule will consume one molecule of ascorbic acid C6H8O6.
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