## Question

###### You have a concentration cell in which the cathode has a silver electrode with 0.10$M \mathrm{Ag}^{+} .$ The anode also has a silver electrode with $\mathrm{Ag}^{+}(a q), 0.050 M \mathrm{S}_{2} \mathrm{O}_{3}^{2-},$ and $1.0 \times 10^{-3} M$ $\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}^{3-}$ . You read the voltage to be 0.76 $\mathrm{V}$ . a. Calculate the concentration of $\mathrm{Ag}^{+}$ at the anode. b. Determine the value of the equilibrium constant for the formation of $\m

You have a concentration cell in which the cathode has a silver electrode with 0.10$M \mathrm{Ag}^{+} .$ The anode also has a silver electrode with $\mathrm{Ag}^{+}(a q), 0.050 M \mathrm{S}_{2} \mathrm{O}_{3}^{2-},$ and $1.0 \times 10^{-3} M$ $\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}^{3-}$ . You read the voltage to be 0.76 $\mathrm{V}$ . a. Calculate the concentration of $\mathrm{Ag}^{+}$ at the anode. b. Determine the value of the equilibrium constant for the formation of $\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}^{3-}$. $$\mathrm{Ag}^{+}(a q)+2 \mathrm{S}_{2} \mathrm{O}_{3}^{2-}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}^{3-}(a q) \quad K=?$$

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