Suppose you have a solution containing both an iron ii salt and an iron iii salt. how would you proceed to identify both Fe 2+ and Fe 3+ in this solution?
See if this will help.
http://www.youtube.com/watch?v=cBy6m_ZlHCc
To identify both Fe2+ and Fe3+ in a solution containing their salts, you can use a few chemical tests and observations. Here is a step-by-step procedure to follow:
1. Prepare a small portion of the solution in a test tube.
2. To identify Fe2+ ions, add a few drops of potassium hexacyanoferrate(II) solution (K4[Fe(CN)6]) to the test tube. If Fe2+ ions are present, you will observe the formation of a dark blue precipitate known as Prussian blue, which confirms the presence of Fe2+ ions.
- The reaction is as follows:
Fe2+ + 3K4[Fe(CN)6] → Fe3[Fe(CN)6]2 + 12K+
3. To identify Fe3+ ions, add a few drops of potassium thiocyanate (KSCN) solution to the remaining portion of the solution in a separate test tube. If Fe3+ ions are present, the solution will turn blood-red, indicating the formation of Fe(SCN)3 (iron thiocyanate) complex.
- The reaction is as follows:
Fe3+ + 3SCN- → [Fe(SCN)3]3-
It's important to note that while potassium hexacyanoferrate(II) can specifically detect Fe2+, potassium thiocyanate can react with both Fe2+ and Fe3+. However, the different colors observed in the reactions will help differentiate between Fe2+ and Fe3+ in the solution.
Remember to perform proper safety precautions while conducting these tests and refer to a reliable source or consult an expert for further guidance.