In a solution, the hydrogen electrode is dipped and $\mathrm{pH}$ of the solution raised from $3 \text{to} 6$ at $25° \mathrm{C}$. The oxidation potential of the cell at $1 \mathrm{atm}$.  

For the cell 

$\mathrm{Pt} \left| {\mathrm{H}}_2(0.4 \mathrm{atm}) \right| {\mathrm{H}}^{+}(\mathrm{pH}=1) \left|\right| {\mathrm{H}}^{+} (\mathrm{pH}=2) | {\mathrm{H}}_2 (0.1 \mathrm{atm}) | \mathrm{Pt}$

the measured potential (in V) at $25° \mathrm{C}$ is:

The cell reaction for the given cell is:

$\mathrm{Pt}\left({\mathrm{H}}_2, 1 \mathrm{atm}\right) | \mathrm{pH}=2 \Vert \mathrm{pH}=3 | \mathrm{Pt}\left({\mathrm{H}}_2, 1 \mathrm{atm}\right)$

Given the data at $25°\mathrm{C}$

$\mathrm{Ag}+{\mathrm{I}}^{-}⟶\mathrm{AgI}+{\mathrm{e}}^{-}$; ${\mathrm{E}}_{\mathrm{OP}}^{\circ }=0.152 \mathrm{V}$

$\mathrm{Ag}⟶{\mathrm{Ag}}^{+}+{\mathrm{e}}^{-}$; ${\mathrm{E}}_{\mathrm{OP}}^{\circ }=-0.800 \mathrm{V}$

What is the value of $\log {\mathrm{K}}_{\mathrm{sp}}$ for $\mathrm{AgI} ? (2.303 \mathrm{RT}/\mathrm{F}=0.059 \mathrm{V})$

The time required to coat a metal surface of $80 {\mathrm{cm}}^2$ with $5\times {10}^{-3} \mathrm{cm}$ thick layer of silver with the passage of $3$ $\mathrm{ampere}$current through a silver nitrate solution is

${\mathrm{d}}_{\text{silver}}=1.05 \mathrm{g} {\mathrm{cm}}^{-3}$ and Molar mass of $\mathrm{Ag}=108 \mathrm{g}$.