Behavious of ferrous oxalate is very complex, I got a pink colour solution during leaching iron oxides using oxalic acid. But I could not able to get
it precipitate ?
I added some alchohal but it not precipitates.
any body has any idea. mnick12 - 31-1-2014 at 20:31
I don't think you have any ferrous oxalate, it is very insoluble in water.blargish - 31-1-2014 at 20:44
I don't think you have any ferrous oxalate, it is very insoluble in water.
When conditions are right ferrous oxalate can stay in solution, as I found out when I tried to synthesize it by mixing ferrous chloride and oxalic
acid. I got a yellow solution, but upon heating the ferrous oxalate began to precipitate. I'm not exactly sure of what caused this.
However, the fact that veerendra got a pink solution suggests that it wasn't ferrous oxalate...mnick12 - 31-1-2014 at 21:44
Ferrous oxalate is only sparingly soluble in water, the soluble compound you generated was likely some sort of transient coordination compound. DraconicAcid - 31-1-2014 at 22:30
Pink? Might there be a manganese impurity in your iron oxide?cyanureeves - 1-2-2014 at 11:07
maybe if you evaporate it you might attain pink crystals or powder,nice either way.blogfast25 - 2-2-2014 at 06:55
But Mn<sup>2+</sup> pink colour is really only apparent at quite high concentrations or in solids like MnCl<sub>2</sub>
hydrate. Also, Mn (II) oxalate is poorly soluble in water, 0.028 g / 100 g water at 20 C acc. Wikipedia.
[Edited on 2-2-2014 by blogfast25]mnick12 - 2-2-2014 at 11:24
Again my guess is some sort of coordination complex, any sort of electron transfer in the d-orbitals produces intensely colored compound.DraconicAcid - 2-2-2014 at 12:18
But Mn<sup>2+</sup> pink colour is really only apparent at quite high concentrations or in solids like MnCl<sub>2</sub>
hydrate. Also, Mn (II) oxalate is poorly soluble in water, 0.028 g / 100 g water at 20 C acc. Wikipedia.
But tris(oxalato)manganate(III) is cherry red- a small amount would make the solution pink.
