oxidation of any chloride ions in the sample). The use of a white background underneath the flask aids in the detecting of the endpoint. Repeat with second sample. Raw Data: 1st weighing, vial and sample 6.042g 2nd weighing, vial and minus half of sample 5.283g3rd weighing, vial 4.524gWeight of samples 0.759g, 0.760gInitial buret reading of first trial 0.00mLFinal buret reading of first trial 14.1mLInitial buret reading of second trial 0.00mLFinal buret reading of second trial 14.4mLCalculations:First trial0.0141L KMnO4 | 0.1001N KMnO4 | 55.85g KMnO4 * 100% = 10.4% Fe 0.759g KMnO4 | 1 mol KMnO4Second trial0.0144L KmnO4 | 0.1001N KmnO4 | 55.85 g KmnO4 * 100% = 10.6% Fe 0.760g KmnO4 | 1 mol KMnO4Discussion:From the equations below it is possible to obtain the oxidation state of reduced ionic form of manganese.5Fe+2 5Fe+3 + 5e- oxidation reactionMnO4-1 + 5e- + 8H+1 Mn+2 + 4H2O reduction reaction5Fe+2 + MnO4-1 + 8H+1 5Fe+3 + Mn+2 + 4H2OThe reduced ionic form of manganese is Mn+2. The equation showsMnO4-1 decomposes into Mn+2, in the reduction equation, which in turn is the reduced ionic form of manganese....
