Calculate the potential of a hydrogen electrode in contact with a solution whose $pH = 10$.

Consider the following electrode processes of a cell: $Cl^{-} \rightarrow \frac{1}{2} Cl_2 + e^{-}$ and $MCl + e^{-} \rightarrow M + Cl^{-}$. If the $EMF$ of this cell is $-1.140 \ V$ and the $E^{\circ}$ value of the cell is $-0.55 \ V$ at $298 \ K$,the value of the equilibrium constant $(K_{sp})$ of the sparingly soluble salt $MCl$ is in the order of:

Calculate the equilibrium constant of the reaction:
$Cu_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Cu^{2+}_{(aq)} + 2Ag_{(s)}$
Given $E^{\Theta}_{cell} = 0.46 \ V$

If $E^{\circ} (Mg^{2+}_{(aq)} \mid Mg_{(s)}) = -2.37 \ V$,what is the potential for the reaction $Mg_{(s)} \longrightarrow Mg^{2+} (0.1 \ M) + 2 \ e^{-}$ at $298 \ K$?

The potential for the given half cell at $298 \ K$ is $(-) \ldots \ldots \ldots \times 10^{-2} \ V.$
$2 H^{+}_{(aq)} + 2 e^- \rightarrow H_{2(g)}$
$[H^{+}] = 1 \ M, P_{H_2} = 2 \ atm$
(Given: $2.303 RT / F = 0.06 \ V, \log 2 = 0.3$)

The reduction potential of a hydrogen electrode at $25^{\circ}C$ is ............... $V$ $(P_{H_2} = 1 \ atm; [H^+] = 0.1 \ M)$.