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If we prepare a solution of $\ce{FeCl2}$ by dissolving solid $\ce{FeCl2}$ powder in water, supposing the bottle of $\ce{FeCl2}$ was left open for sufficient time, is it possible for $\ce{FeCl2}$ to have oxidised to $\ce{FeCl3}$? I can't find a suitable reaction for this excecpt one which includes $\ce{HCl}$ which was definitely not present when preparing the mixture.

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    $\begingroup$ Yes, it is very common. You actually have to protect Fe(II) solution from air when you do experiments if oxidation is something you want to avoid. $\endgroup$ – Greg Jun 6 '17 at 4:03
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The yellow/brown color you are seeing in the solution of $\ce{FeCl2}$ is due to formation of various types of hydrated iron oxide and not iron(III) chloride. They may include both the anhydrous($\ce{FeOOH}$) or the monohydrate($\ce{FeOOH.H2O}$) often referred to as ferric hydroxide($\ce{Fe(OH)3}$). They are generally yellow to brown in color. The reaction is given here:

$$\ce{4FeCl2 + 6H2O + O2 → 4FeO(OH) + 8HCl}$$

Reaction between iron chloride (II), water and oxygen(moisture) to form iron metahydroxide(Iron(III) oxide-hydroxide) and hydrogen chloride. The reaction takes place at reflux.

Moreover, if you further heat iron chloride in oxygen at 450-480℃, iron oxide will form.

References(all pdf links)

  1. https://www.google.co.in/url?sa=t&source=web&rct=j&url=http://www.jieas.com/fvolumes/vol081-5/3-5-11.pdf&ved=0ahUKEwidw86XsqjUAhXLM48KHRbODMkQFggjMAE&usg=AFQjCNGeU9yaSSIfaQ51Tcclo0sik8pjfA&sig2=R0kK4DzQp0qktLPHSW0afQ
  2. https://www.google.co.in/url?sa=t&source=web&rct=j&url=http://www.gfredlee.com/SurfaceWQ/StummOxygenFerrous.pdf&ved=0ahUKEwidw86XsqjUAhXLM48KHRbODMkQFgg-MAM&usg=AFQjCNEl5N7ZQKTiJS1WvERl0gz8fBXirQ&sig2=aCnvMH456QBuY-pTdDRgrg
  3. https://www.google.co.in/url?sa=t&source=web&rct=j&url=http://repository.kulib.kyoto-u.ac.jp/dspace/bitstream/2433/77056/1/chd061_5-6_335.pdf&ved=0ahUKEwidw86XsqjUAhXLM48KHRbODMkQFghMMAQ&usg=AFQjCNHecL15xq-93ZrwAJ5i8riSyMrVTQ&sig2=cQwDCmjJV6i_QOOYtzYOJQ
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  • $\begingroup$ That's interesting... I guess what I've learnt in school is only for the Cambridge Advanced Levels, which is probably the simplified explanation. Your explanation seems credible and convincing as well. $\endgroup$ – Tan Yong Boon Jun 6 '17 at 9:52
  • $\begingroup$ But no solid is formed during the oxidation process... Wouldn't the hydrated iron (III) oxide-hydroxide give an insoluble precipitate. From my own observations in the laboratory, I have never seen any precipitate in a solution of yellow iron (III) chloride solution. How would you explain the absence of a ppt? $\endgroup$ – Tan Yong Boon Jun 6 '17 at 9:56
  • $\begingroup$ @TanYongBoon iron(III) hydroxide is indeed insoluble in neutral and basic pH and precipitates in the bottom of the solution(according to 1st link). However, the ferrous chloride solution present in the laboratory has somewhat an acidic pH for which the the hydrated iron oxide or iron(III) hydroxide solubilize in the solution and thus not get any precipitate. $\endgroup$ – Nilay Ghosh Jun 6 '17 at 11:22
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$\ce{Fe^2+ -> Fe^3+ + e- E^o = +0.771 V}$

$\ce{O2 + 2H2O + 4e- -> 4OH- E^o = +0.40 V }$

Thus, oxidation of iron (II) to iron (III) ions is feasible with atmospheric oxygen as the overall cell potential for the reaction is +1.171 V and it does occur at a reasonably observable rate.

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