The standard cell potential $E^o$ for the reaction $aA + bB \to cC + dD$ is related to the equilibrium constant $K_c$ by the expression:

If a hydrogen electrode is dipped in two solutions of $pH = 3$ and $pH = 6$ and a salt bridge is connected,the e.m.f. of the resulting cell is ............ $V$.

Give the $E_{cell}$ equation for the general reaction: $aA + bB \to cC + dD$.

The reduction potential of a hydrogen half-cell will be positive if:

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:

What will be the reduction potential of $Cu$ in an aqueous solution with $pH = 12$? Given that the $K_{sp}$ of $Cu(OH)_2$ is $1 \times 10^{-19}$ and $E^o_{Cu^{2+}/Cu} = 0.34 \ V$.