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When you mix aqueous iron(III) nitrate and potassium thiocyanate together you get a red solution. Then if you add sodium fluoride, the red colour disappears.

This is basically because the $\ce{Fe(SCN)^2+}$ ions are red, but $\ce{FeF^2+}$ ions are colourless.

I get Le Chatelier's principle in that, the more iron ions that are stolen by the fluoride, the less $\ce{Fe(SCN)^2+}$ ions there will be because they keep dissociating etc.

The thing I wonder about is why the fluoride atoms get all the iron. I can think of a couple of potential reasons for this, but I don't know which, if any of them, are true, even after googling a fair bit.

Could it be the case that iron is a lot more attracted to fluoride than thiocyanate? Or that the fluoride reaction isn't reversible? And if either of those is true, can this experiment be seen as evidence for that?

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  • $\begingroup$ Well, I guess Fe(III) (aq) is "hard" enough to prefer F- from SCN- $\endgroup$
    – Mithoron
    Commented Apr 7, 2017 at 15:22

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I found this on the MEL science website (https://melscience.com/US-en/articles/fake-chemical-cut/)

"Adding sodi­um flu­o­ride de­stroys the iron(III) thio­cyanate com­plex­es, and col­or­less hex­aflu­o­ro­fer­rate(III) [FeF₆]³¯ ions form. Fe(CNS)₃ + 6NaF→Na₃[FeF₆] + 3NaC­NS"

Seems that it may create this hexafluoriferrate ion instead... just thought I'd add to this discussion. I was actually just trying to find out a bit more about this reaction myself. AP Chem teacher here :)

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