Chapter 11, Problem 69E

You have a concentration cell in which the cathode hasa silver electrode with 0.10 M ${\text{Ag}}^{\text{+}}$ . The anode also hasa silver electrode with $\text{Ag+(}aq\text{), 0}\text{.050}M{\text{S}}_{\text{2}}{\text{O}}_{\text{3}}{}^{\text{2–}}\text{, and 1}{\text{.0×10}}^{\text{-3}}M{\text{Ag(S}}_{\text{2}}{\text{O}}_{\text{3}}{\text{)}}_{\text{2}}{}^{\text{3–}}$ . You read the voltage to be0.76 V.
a. Calculate the concentration of ${\text{Ag}}^{\text{+}}$ at the anode.
b. Determine the value of the equilibrium constant forthe formation of ${\text{Ag(S}}_{\text{2}}{\text{O}}_{\text{3}}{\text{)}}_{\text{2}}{}^{\text{3–}}$ .
${\text{Ag}}^{\text{+}}\text{(}aq{\text{)+2S}}_{\text{2}}{\text{O}}_{\text{3}}{\text{2}}^{\text{–}}\text{(}aq\text{)}\rightleftharpoons {\text{Ag(S}}_{\text{2}}{\text{O}}_{\text{3}}{\text{)}}_{\text{2}}{}^{\text{3–}}\text{(}aq\text{)}K\text{=?}$