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chloric1
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Registered: 8-10-2003
Location: GroupVII of the periodic table
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It’s not critical so long as you have a slight excess of acid. You will be adding more iron into solution anyways.
As long as metallic iron is present ferric will be reduced to ferrous in acid solution
Fellow molecular manipulator
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chloric1
International Hazard
Posts: 1070
Registered: 8-10-2003
Location: GroupVII of the periodic table
Member Is Offline
Mood: Stoichiometrically Balanced
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Quote: Originally posted by woelen  | | Recovering oxidized iron(II) sulfate is very difficult and is not worth the effort. If you want an iron(II) salt, then next time I would purchase
Mohr's salt, Fe(NH4)2(SO4)2.12H2O. Mohr's salt is MUCH more stable in air than ferrous sulfate. It is not so easily oxidized. |
Sorry but no. It’s so easy. I have purchased “copperas” from a fertilizer co-op store, took it home, and made up 20% sulfuric acid solution
added the brownish yellow iron salt and boiler with regular nails for about an hour or two and let it cool and got beautiful blue green crystals
Fellow molecular manipulator
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