Any way we can be sure this is not Fe2O3 (iron III Oxide)? Wikipedia's article on Iron(II) carbonate currently states reaction of Iron(III) (ferric) ions with carbonate ions result in the production of iron(III) oxide.. or were these Iron II ions you reacted? Thanks for your videos!
There will be some contamination with iron(III) hydroxide as carbonate is in equilibrium with hydroxide (there is always some amount of hydroxide present in water due to autolysis, but carbonate shifts the equilibrium to the hydroxide side). This produces some iron(II) hydroxide which is prone to oxidation - iron(III) hydroxide is itself acidic and will neutralize some of the carbonate. You can this use bicarbonate instead - either directly or by saturating the carbonate solution saturated with CO2. This will give you cleaner iron(II) carbonate. Maybe using even less alkaline (bi)carbonate, such as that of magnesium will improve the results even more. The key is promoting displacement over acid-base reaction. There might be some basic salts present depending on you iron(II) source - using sulfate is preferred over chloride to minimize hydrolysis. Ferrous ammonium sulfate might give you good results as the acidity of ammonium stabilizes the divalent iron against oxidation. Adding dilute bicarbonate to dilute iron(II) solution slowly is also advantageous as this won't bump the pH too quickly.
"Thank you, @LiborTinka, for the insightful information! I appreciate the clarification on the equilibrium dynamics with hydroxide and the recommendation to use bicarbonate for obtaining cleaner iron(II) carbonate. I'll definitely consider experimenting with less alkaline bicarbonate for potential improvements. The tips on the choice of iron(II) source and sulfate over chloride are also helpful. I'll keep in mind the gradual addition of dilute bicarbonate to control pH changes. Thanks again for sharing your expertise!"
Any way we can be sure this is not Fe2O3 (iron III Oxide)? Wikipedia's article on Iron(II) carbonate currently states reaction of Iron(III) (ferric) ions with carbonate ions result in the production of iron(III) oxide.. or were these Iron II ions you reacted? Thanks for your videos!
There will be some contamination with iron(III) hydroxide as carbonate is in equilibrium with hydroxide (there is always some amount of hydroxide present in water due to autolysis, but carbonate shifts the equilibrium to the hydroxide side). This produces some iron(II) hydroxide which is prone to oxidation - iron(III) hydroxide is itself acidic and will neutralize some of the carbonate.
You can this use bicarbonate instead - either directly or by saturating the carbonate solution saturated with CO2. This will give you cleaner iron(II) carbonate. Maybe using even less alkaline (bi)carbonate, such as that of magnesium will improve the results even more.
The key is promoting displacement over acid-base reaction.
There might be some basic salts present depending on you iron(II) source - using sulfate is preferred over chloride to minimize hydrolysis. Ferrous ammonium sulfate might give you good results as the acidity of ammonium stabilizes the divalent iron against oxidation. Adding dilute bicarbonate to dilute iron(II) solution slowly is also advantageous as this won't bump the pH too quickly.
"Thank you, @LiborTinka, for the insightful information! I appreciate the clarification on the equilibrium dynamics with hydroxide and the recommendation to use bicarbonate for obtaining cleaner iron(II) carbonate. I'll definitely consider experimenting with less alkaline bicarbonate for potential improvements. The tips on the choice of iron(II) source and sulfate over chloride are also helpful. I'll keep in mind the gradual addition of dilute bicarbonate to control pH changes. Thanks again for sharing your expertise!"
When I do this I somehow get iron hydroxide which is a strong blue/green color. I havent yet figured out why. (Maybe the base is too concentrated).
Can I Use CaCO3 instead of Sodium Carbonate? Why can't I find a video of FeCO3 using CaCO3? Is it because the additional CaCO3 is not soluble?
Yes brother you can use CaCO3.
But I will recommend you to use NaCO3
@@Molybdenum-h Do you recommend Na2CO3 just because it is soluble in water and the excess will not contaminate the result?
Yes. You can use CaCO3
Hi
Yes