Hydrogen Peroxide → Copper
Reaction equation
[Cu:1].O.OO.O=O.[CH3:7][S:8]([OH:11])(=[O:10])=[O:9]>>[CH3:7][S:8]([O-:11])(=[O:10])=[O:9].[Cu+2:1].[CH3:7][S:8]([O-:11])(=[O:10])=[O:9].[Cu:1]Participants
7
[Cu:1].O.OO.O=O.[CH3:7][S:8]([OH:11])(=[O:10])=[O:9]>>[CH3:7][S:8]([O-:11])(=[O:10])=[O:9].[Cu+2:1].[CH3:7][S:8]([O-:11])(=[O:10])=[O:9].[Cu:1]100 g copper wire scrap was introduced into an aqueous solution that contained 300 g methanesulfonic acid; this was brought to approximately 0.7 L by the addition of ion-exchanged water; and, while heating to 80° C., 30% aqueous hydrogen peroxide was intermittently added in 10 mL portions while monitoring the status of the reaction. Once a certain amount had been added, decomposition of the hydrogen peroxide began and oxygen gas was generated and this caused oxidation of the copper and its gradual dissolution in the methanesulfonic acid. Aqueous hydrogen peroxide was further added when the reaction had calmed. After several hours the copper wire was finally completely dissolved and an aqueous copper methanesulfonate solution with a copper concentration of 100 g/L was produced. The pH of the obtained aqueous copper methanesulfonate solution was 2.5.
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