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The Nernst equation: Consider the follow...

The Nernst equation: Consider the following galvanic cell
`Pb(s) | Pb^(2+)(aq.) || Ag^(2+)(aq.) | Ag(s)`
(a) What is the quantitative change in the cell voltage on increas-ing the ion concentrations in the anode compartment by a factor of `10`?
(b) What is the quantitative change in the cell voltage on increas-ing the ion concentration in the cathode compartment by a factor of `10`
Strategy: The conventional notation of the cell tells us that lead is the anode while silve is the cathode. Therfore, the cell reaction is
`Pb(s) + 2Ag^(+)(aq.) rarr Pb^(2+)(aq.) + 2Ag(s)`
The cell potantial (at `25^(@)C`) is given by the Nernst equation, where `n = 2` and `Q = C_(Pb^(2+))//C_(Ag^(+))`:
`E_("cell") = E_("cell")^(@)-(0.0592 V)/(n) "logQ"`
`E_("cell")^(@)-(0.0592 V)/(n) "logQ" C_(Pb^(2+))/C_(Ag^(+))^(2)`

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