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### 6 Cards in this Set

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 Compounds with:1) High oxidation states?2) Low oxidation states? 1) Usually good oxidising agents.2) Usually good reducing agents. Fe (II) is used to: Reduce manganate and dichromate (it's a reducing agent). The acid we use:1) Needs to be?2) It can't be?3) So we use? 1) It needs to be strong to suplpy enough H+'s.2) It cannot be a reducing agent or an oxidising agent.3) We use Dilute sulphuric acid. Fe (II) with Manganate:1) To derive the redox equation?2) The colour of the end point? 1) Use the two half equations.• MnO4¯ → Mn^2+• Fe^2+ → Fe^3+2) Purple. Fe (II) with Dichromate:1) To derive the redox equation?2) The colour of the end point? 1) We use the two half equations.• Cr2O7^2¯ → Cr^3+• Fe^2+ → Fe^3+2) Green Cr^3+. To calculate the conc. of a reagent from a titration:– 4 steps? 1) Write out the full balanced redox equation.2) Calculate the moles of anything you can.3) Use the ratios to find the moles of what you're looking for.4) Use the C = n/V to get your concentration. If a mass is given, m/Mr = n.