The reaction below competes with the formation of the FeSCN2+ complex
Fe3+(aq) + 4Cl-(aq)↔ FeCl-4(aq)
Yellow Colorless
Explain what would happen to the color of a dilute solution containing FeCl-4 if
A. You added a solution containing silver ion, Ag+ (silver ion reacts with chloride ion in solution to form the precipitate AgCl.)
B. You added a solution of sodium chloride, NaCl.
C. You added concentrated HCl.
D. You added concentrated H3PO4
Fe3+(aq) + 4Cl-(aq)↔ FeCl-4(aq)
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Your question is not quite clear. Please make a search on iron rhodanide complexes and you will fing plenty of information since it's a very common reaction.
http://www.google.com/#hl=en&source=hp& ... 0d3c90c6fc
Obviously, othe anions will compete with rhodanide. When you add them (chloride in your case), the rhodanide gets substituted and the salt is loosing color. When you remove them by Ag+ the color returns.
Make sure check out this ref http://en.wikipedia.org/wiki/Thiocyanate
http://www.google.com/#hl=en&source=hp& ... 0d3c90c6fc
Obviously, othe anions will compete with rhodanide. When you add them (chloride in your case), the rhodanide gets substituted and the salt is loosing color. When you remove them by Ag+ the color returns.
Make sure check out this ref http://en.wikipedia.org/wiki/Thiocyanate
Remember safety first! Check MSDS and consult with professionals before performing risky experiments.