Question
The value of $K_{\text {sp }}$ for $\mathrm{AgBr}$ is $5.4 \times 10^{-13}$. What will be the potential of a cell constructed of a standard hydrogen electrode as one half-cell and a silver wire coated with AgBr dipping into $0.10 M \mathrm{HBr}$ as the other half-cell. For the $\mathrm{Ag} / \mathrm{AgBr}$ electrode, $\operatorname{AgBr}(s)+e^{-} \rightleftharpoons \mathrm{Ag}(s)+\mathrm{Br}^{-}(a q) \quad E_{\mathrm{A}_{\mathrm{F}} \mathrm{B}_{t}}^{\circ}=+0.070 \mathrm{~V}$
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0592}{n} \log Q\] where \(E\) is the cell potential, \(E^{\circ}\) is the standard cell potential, \(n\) is the number of electrons transferred in the redox reaction, and \(Q\) is the reaction quotient. Show more…
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The value of $K_{\mathrm{g}}$ for $\mathrm{AgBr}$ is $5.4 \times 10^{-13}$. What will be the potential of a cell constructed of a standard hydrogen electrode as one half-cell and a silver wire coated with AgBr dipping into $0.10 M \mathrm{HBr}$ as the other halfcell. For the $\mathrm{Ag} / \mathrm{AgBr}$ electrode, $$ \begin{aligned} \mathrm{AgBr}(s)+e^{-} \rightleftharpoons \mathrm{Ag}(s)+\mathrm{Br}^{-}(a q) & \\ E_{\mathrm{AgBr}}^{\circ} &=+0.070 \mathrm{~V} \end{aligned} $$
A galvanic cell has a silver electrode in contact with 0.050 $\mathrm{M} \mathrm{AgNO}_{3}$ and a copper electrode in contact with 1.0 $\mathrm{M} \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}$ (a) Write a balanced equation for the cell reaction, and calculate the cell potential at $25^{\circ} \mathrm{C}$ . (b) Excess $\mathrm{NaBr}(a q)$ is added to the AgNO_ solution to pre- cipitate AgBr. What is the cell potential at $25^{\circ} \mathrm{C}$ after the precipitation of AgBr if the concentration of excess $\mathrm{Br}^{-}$ is 1.0 $\mathrm{M}$ ? Write a balanced equation for the cell reaction under these conditions. $\left(K_{\mathrm{sp}} \text { for AgBr at } 25^{\circ} \mathrm{C} \text { is }\right.$ $5.4 \times 10^{-13}$ ) (c) Use the result in part (b) to calculate the standard reduction potential $E^{\circ}$ for the half-reaction $$\operatorname{Ag} \operatorname{Br}(s)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)+\mathrm{Br}^{-}(a q)$$
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