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Lab: Analysis of Hydrogen Peroxide SolutionsFill a burette with 50 mL of 0.2M potassium permanganate solution. Add 10 mL of NEW hydrogen peroxide and 2 mL of 6M sulfuric acid to a flask. Titrate the hydrogen peroxide with the KMnO4 solution to the purple endpoint of excess MnO4- ion.
Questions:(a) Volume of potassium permanganate used in each titration (mL):50mL(b) The volume of potassium permanganate required to titrate 10 mL of the new hydrogen peroxide (mL):20mL(c) Calculate the concentration of H2O2 from the volume of KMnO4 used and the stoichiometry of the reaction (MW of H2O2 is 34.01).
In these calculations I got lost.-I found 0.12655 mol KMnO4. Is this the amount in mol of KMnO4 which reacted? So now how I get the concentration of the H2O2?-2(C2x0.02L)KMnO4=5(34.01xV1)H2O2. What is C2 and V1?
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In the reaction MnO4- + 8H+ + 5e- ⇔ Mn2+ + 4H20, the manganese in 3.95 grams of KMnO4 is reduced to Mn2+. How many coulombs of charge must have been transferred to the permanganate ion.
What mass of barium sulfate is produced when 100.0 mL of a 0.100 M solution of barium chloride is mixed with 100.0 mL of a 0.100 M solution of iron(III) sulfate.
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