Gold exists in two common positive oxidation states, +1 and +3. The standard reduction potentials for these oxidation states are
Au+(aq) + e-→ Au(s) E°red = +1.69 V
Au3+(aq) + 3 e-→ Au(s) E°red = +1.50 V
(a) Can you use these data to explain why gold does not tarnish in the air? (b) Suggest several substances that should be strong enough oxidizing agents to oxidize gold metal. (c) Miners obtain gold by soaking gold-containing ores in an aqueous solution of sodium cyanide. A very soluble complex ion of gold forms in the aqueous solution because of the redox reaction
4 Au(s) + 8 NaCN(aq) + 2 H2O(l) + O2(g)→ 4 Na[Au(CN)2](aq) + 4 NaOH(aq)
What is being oxidized and what is being reduced in this reaction? (d) Gold miners then react the basic aqueous product solution from part (c) with Zn dust to get gold metal. Write a balanced redox reaction for this process. What is being oxidized, and what is being reduced?
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