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Registered Member #5436
Joined: Sun Jun 24 2012, 01:44AM
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What would be the products of those reactions, in order?
Adding the peroxide to the spent ferric chloride produces a dark greenish yellow liquid, like cola only it stains greenish yellow. Adding aluminum to that produces a exothermic reaction where the al is disolved and a flammable gas is produced. Every substance from each step dissolves copper well.
Registered Member #5980
Joined: Wed Aug 01 2012, 05:47PM
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I am not certain what you mean by "spent" ferric chloride. Were you etching something?
From the Iron (III) chloride wikipedia page: When dissolved in water, iron(III) chloride undergoes hydrolysis and gives off heat in an exothermic reaction. The resulting brown, acidic, and corrosive solution is used as a flocculent in sewage treatment and drinking water production, and as an etchant for copper-based metals in printed circuit boards. Anhydrous iron(III) chloride is a fairly strong Lewis acid, and it is used as a catalyst in organic synthesis.
Would the iron chloride dissolve in plain water? Peroxide may be unnecessary.
Aluminum naturally reacts with water to release hydrogen. Under normal conditions a film of dull grey aluminum oxide forms on the surface of aluminum and protects the underlying aluminum. The spent ferric chloride likely removes that layer of aluminum oxide, which allows the underlying aluminum to dissolve - likely into aluminum 3+.
Iron(III) chloride is a mild oxidising agent, for example, it is capable of oxidising copper(I) chloride to copper(II) chloride. FeCl3 + CuCl → FeCl2 + CuCl2
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Ferric chloride+copper+h2o2+aluminum
