Chapter 19, Problem 101FP

Consider the following electrochemical cell:

   $\text{Pt}\left(\text{s}\right){\text{|H}}_{\text{2}}\left(\text{g,}\text{1bar}\right){\text{|H}}^{\text{+}}\left(\text{1M}\right){\text{||Ag}}^{\text{+}}\left(\text{xM}\right)\text{|Ag}\left(\text{s}\right)$

a. What is $E_{\text{col}}^{°}$ -that is, cell potential when $\left[A{g}^{+}\right]=1\text{M}$ ?

b. Use the Nernst equation to write an equation for $E_{\text{col}}$ when $\left[A{g}^{+}\right]=x$ .

c. Now imagine titrating 50.0 mL of 0.0100 M ${\text{AgNO}}_{\text{2}}$ in the cathode half-cell compartment with 0.0100 M Kl. The titration reaction is $\begin{array}{l}{\text{Ag}}^{\text{+}}\left(\text{aq}\right)+{\text{I}}^{\text{-}}\left(\text{aq}\right)\to \text{AgI}\left(\text{s}\right)\\ \end{array}$ Calculate $\left[A{g}^{+}\right]$ and then $E_{\text{col}}$ after addition of the following volumes of 0.0100 M Kl (i) 0.0mL; (ii) 20.0mL: (Mi) 49.0 mL. (iv) 50.0 mL (v) 60.0 mL.

d. Use the results of part (c) to sketch the titration curve of ${\text{E}}_{\text{col}}$ versus volume of titrant.