consider the following voltaic cell Pt | OCl- (aq) | Cl- (aq) || SO4^-2 (aq) | S

Question

consider the following voltaic cell

Pt | OCl- (aq) | Cl- (aq) || SO4^-2 (aq) | S2O8^-2 (aq) | Pt

What pH would the solution need to be to drop the voltage by 10% while all ion concentrations are 0.010M?

The standard reduction potentials of the peroxydisulfate ion and the hypochlorite ion are 2.01V and 0.90V respectively. I calculated the overall voltage of the cell to be 2.91V (I'm not sure if this bit is necessary)

This was all the info I was provided with. Please explain all the steps. Thank you!

Explanation / Answer

Cl-    +    H2O      =    ClO-   + 2[H+] + 2e              anode   E0red = +0.90 V

2 S2O82-    + 2e    = SO42-                                     cathode   E0red = +2.05 V

Cl-    + H2O + 2 S2O82-    = ClO-   + 2[H+] + SO42-   Ecell = +2.05

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