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4.Calculate the number of moles of MnO4in 20.10 mL of .020 5.Calculate the number of moles of hydrogen peroxide needed to react with 20.10 mL of 0.020 MKMnO46.Hydrogen Peroxide solution sold in the grocery store is 3%(by mass). Assuming a densityof 1.0 g/mL, calculate the molarity of 3.0% H2O2.
1.Measure out precisely 10 mL of 0.3% hydrogen peroxide solution from the dispensing burette your teacher has prepared into a 250 mL Erlenmeyer Flask. Should you miss the 10.00 mL mark, just record the volume of your sample exactly.2.Measure out approximately 10 M of 4.5Msulfuric acid, H2SO4, solution from dispensing burette your teacher has prepared into the flask containg the 0.3% hydrogen peroxide solution. Caution:H2SO4is a strong acid, and should be handled with care.3.Use a graduated cylinder to meaure out approximately 25 mL of water and add it to the beaker as well.4.Set up a ring stand, a burette clamp, and a burette to conduct the titration. Rinse and fill the 50 Ml burette with 0.0200 M MnO4-solution. CAUTION: Handle the KMnOsolution with care; it has been mixed the H2SO4 which can cause painful burns if it comes in contact with the skin.4Equations:5H202 + @MnO4 + 6H – 5O2 + 2Mn + 8H2OOx: Mno4 + 8H + 5e- Mn + 4H2ORed: H2O2 – 2H + O2 + 2eGraphs:Insufficient dataPost-Lab Questions: