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What happens when you connect two silver wires immersed in 0.1M HCl to the poles of a 1.5 V battery and passing current for some time? What are the possible reactions that can occur at the anode and cathode? Which reactions will be more favorable? Would silver chloride form at either electrode? Why or why not?
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One Response
reactions that could happen @ the cathode & their reduction potentials:
2 H+ & 2 e- –> H2 …….. ….. …. Eo = 0.00 volts
2 H2O & 2 e- –> H2 & 2 OH- …. .. Eo = -0.83 volts
reactions that could happen @ the anode, & their oxidation potentials:
Ag –> Ag+ & 1 e- …. … .Eo = – 0.799 volts
2Cl- –> Cl2 & 2 e- …….. … Eo = – 1.359 volts
2 H2O –> O2 & 4 H+ & 4 e- Eo = – 1.23 volts
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the most favorable reactions require the least voltage:
2 H+ & 2 e- –> H2 (@ cathode) Eo = 0.00 volts
Ag –> Ag+ & 1 e- (@ anode) Eo = – 0.799 volts
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yes AgCl should form @ the anode where Ag+ ions being produced combine with Cl- ions from HCl,
because Ag is the easiest to be oxidized, easier than oxidizing oxygen in the water, or chloride ion
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What happens when you connect two silver wires immersed in 0.1M HCl to the poles of a 1.5 V battery and passing current for some time?
Ag gets oxidized @ the anode, producing Ag+ ions, which then precipitate as AgCl, while H2 gas is being produced at the cathode from the H+ ions being reduced