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6 Cards in this Set

  • Front
  • Back
  • 3rd side (hint)
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.