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1) Calculate the value of the solubility product constant for PbSO4 from the half-cell potentials.
PbSO4(s) + 2e- â Pb(s) + SO42-(aq) Eº = -0.397 V
Pb2+ + 2e- â Pb(s) Eº = -0.148 V
2) Use standard reduction potentials (shown below) to calculate the potential of a nickel-cadmium cell that uses a basic electrolyte that has a 0.6 M hydroxide concentration.
Cd(OH)2(s) + 2e- â Cd(s) + 2OH-(aq) Eº = -0.83 V
NiO(OH)s) + H2O(l) + e- â Ni(OH)2(s) + OH-(aq) Eº = 0.52 V
1) Calculate the value of the solubility product constant for PbSO4 from the half-cell potentials.
PbSO4(s) + 2e- â Pb(s) + SO42-(aq) Eº = -0.397 V
Pb2+ + 2e- â Pb(s) Eº = -0.148 V
2) Use standard reduction potentials (shown below) to calculate the potential of a nickel-cadmium cell that uses a basic electrolyte that has a 0.6 M hydroxide concentration.
Cd(OH)2(s) + 2e- â Cd(s) + 2OH-(aq) Eº = -0.83 V
NiO(OH)s) + H2O(l) + e- â Ni(OH)2(s) + OH-(aq) Eº = 0.52 V
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Keith LeannonLv2
15 Sep 2019
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