zoomer - 31-3-2005 at 05:22
If solid iron was placed in a solution containing both sulfate & carbonate ions, would the iron attract either ion preferencially? Or would both
interact equally with the iron? What if the iron was not solid but in solution?
Thanks!
Z
JohnWW - 31-3-2005 at 05:53
Fe(II) would immediately precipitate out as FeCO3. This is found in nature as cerussite, the product of partial oxidation, then reaction with CO2, of
iron sulfide mineral deposits (e.g. pyrite or marcasite) under conditions insufficient to result in Fe(III).
With Fe(III), the reaction with carbonate is less clear: Fe(OH)3 is more likely to precipitate out, although at low temperatures a basic carbonate
with a formula like (FeO)2CO3 could result. This is a similar situation to the reaction of Al(III) with carbonate.
sparkgap - 31-3-2005 at 05:56
Huh? Would the solid iron form ferrous or ferric ions upon immersion in water?
I'm thinking the iron will rust first... 
sparky (*_*)
Darkblade48 - 31-3-2005 at 13:42
I would imagine that the iron would form both Fe+2 and Fe+3 ions upon contact with water, and you'd end up with a mixture of products.
Though iron itself doesn't rust that fast in water...now add some salt and hook it up as the anode and pass some current through it....
zoomer - 31-3-2005 at 16:20
So would any metal take the sulfate and leave the carbonate? (Other than copper)
12AX7 - 31-3-2005 at 18:13
Only one where the sulfate is less soluble than the carbonate. Strontium and barium ions are candidates.
Tim