By Thomas B. Drew (ed.), Giles R. Cokelet (ed.), John W. Hoopes (ed.), Theodore Vermeulen (ed.)
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Extra info for Advances in Chemical Engineering, Vol. 9
The presence of iron and/or sulfur in practically all of the ores used for metal recovery provides a readily available source of leaching reagents in the presence of water. Acid solutions of iron sulfate and sulfuric acid are produced by natural processes and are readily available in the streams 24 RENATO G. BAUTISTA near most mining operations, or in the mine waters themselves. The ability of acidic ferric sulfate and sulfuric acid to oxidize most of the metal sulfides and oxides during the process of dissolution is wdl known.
Lead silicate can be trrated by acid treatment. The pretreated material is leached under ambient conditions, yielding pregnant liquor containing up to 100 gm/liter P b and n barren residue. The precipitation of lead can be carried out by electrolysis to produce the metal, by removal of free ammonia, or by heating of the supersaturated leach liquor to produce ammonium sulfate, monobasic lead sulfate or a mixture of the two. The remaining ammoniacal ammonium solution is recycled to the leaching stage after removal of other accumulated metals such as copper and zinc.
Since the precipitation of ferric iron as sulfate in the copper mine waste dump must be minimized, the practice at Kennecott is to add sulfuric acid to the leaching solution to suppress the biological oxidation of ferrous iron. Other investigators (14, T3) contend that the bacteria biologically oxidize the ferrous to the ferric state as sulfate, which in turn attacks the metal sulfides ores, resulting in both the dissolution of the metal and the oxidation of the sulfide. In the process the ferric iron reduces back to the ferrous state.
Advances in Chemical Engineering, Vol. 9 by Thomas B. Drew (ed.), Giles R. Cokelet (ed.), John W. Hoopes (ed.), Theodore Vermeulen (ed.)