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    Ksp of Pb3(AsO4)2

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    The following cell was found to have a potential of 0.416 V. Calculate the k for Pb3(ASO4)2.

    Pb3(s)| Pb3(AsO)2(saturated) AsO4^3-(1.00x10^-3 M) || S.H.E.

    Pb^2+ +2e- <---> Pb(s) E^o = -0.126 V

    H3AsO4 + 2H+ + 2e- <---> H3AsO3 + H2O E^o = 0.559 V

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    https://brainmass.com/chemistry/inorganic-chemical-reactions/calculating-solubility-product-constant-567065

    Solution Preview

    The oxidation half-reaction of the cell is the oxidation of Pb to Pb2+, and the reduction half reaction is the SHE half reaction.
    OHR: Pb(s) <=> Pb2+(aq) + 2e- E° = 0.126 V
    RHR: 2H+ + 2e- <=> H2O E° = 0.000 V
    Overall cell ...

    Solution Summary

    This solution shows the calculation of solubility product constant from electrochemical data.

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