The standard reduction potential for the following two reactions are given by
$\begin{array}{ll}\mathrm{AgCl}+{\mathrm{e}}^{-}\to \mathrm{Ag} \left(\mathrm{s}\right)+{\mathrm{Cl}}^{-} \left(\mathrm{aq}\right);& {\mathrm{E}}^0=0.22 \mathrm{V}\end{array}$

$\begin{array}{ll}{\mathrm{Ag}}^{+} \left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\to \mathrm{Ag} \left(\mathrm{s}\right);& {\mathrm{E}}^0=0.80 \mathrm{V}\end{array}$

The solubility product of $\mathrm{AgCl}$ under standard condition will be

Calculate the cell potential of following $\mathrm{Pt} \left(\mathrm{s}\right)\left|{\mathrm{H}}_2\left(\mathrm{g}\right)\left(0.1\mathrm{bar}\right)\right|\overline{)\mathrm{BOH} \left(0.1\mathrm{M} \mathrm{aq}\right)}\left|\mathrm{HA} \left(0.1\mathrm{M}\right)\right|{\mathrm{H}}_2\left(\mathrm{g}\right)$$\overline{)\left(1\mathrm{bar}\right)}\mathrm{Pt}$ 

Given, ${\mathrm{K}}_{\mathrm{a}}=\left(\mathrm{HA}\right)={10}^{-7},{\mathrm{K}}_{\mathrm{b}}\left(\mathrm{BOH}\right)={10}^{-5}$.

Which of the following expression(s) represent the voltage of cell at $298 \mathrm{K}?$

$\mathrm{Ag}\left(\mathrm{s}\right)\left|\mathrm{Ag}\right|$ (saturated solution) $\overline{)|{\mathrm{Ag}}_2{\mathrm{C}}_2{\mathrm{O}}_4}$ (saturated solution) $\overline{)\mathrm{Ag} \left(\mathrm{s}\right)}$

In the following electrochemical cell: $\mathrm{Pt} \overline{) {\mathrm{H}}_2} \left(\mathrm{x} \mathrm{atm}\right) \overline{) {\mathrm{H}}^{+} }\left(\mathrm{pH}=\mathrm{y}\right) \Vert {\mathrm{Zn}}^{2+} \left(\mathrm{z} \mathrm{M}\right) \overline{) \mathrm{Zn}}$

${\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}={\mathrm{E}}_{\text{cell }}.$ This will be possible when