232-- The electromotive force ($\mathrm{E^\circ}$) of the reaction: $\mathrm{M(s) + 2Ag^+(aq) \rightarrow M^{2+}(aq) + 2Ag(s)}$ is equal to $+1.56$ V and $\mathrm{E^\circ}$ of the electrode M is $+0.80$ V. The $\mathrm{E^\circ}$ of electrode M is $+0.80$ V, the potential of cation $\mathrm{Ag^+(aq)}$ is .............. and the cation $\mathrm{M^{2+}(aq)}$ is ..............
\textbf{232--} The electromotive force ($\mathrm{E^\circ}$) of the reaction: $\mathrm{M(s) + 2Ag^+(aq) \rightarrow M^{2+}(aq) + 2Ag(s)}$ is equal to $+1.56$ V and $\mathrm{E^\circ}$ of the electrode M is $+0.80$ V. The $\mathrm{E^\circ}$ of electrode M is $+0.80$ V, the potential of cation $\mathrm{Ag^+(aq)}$ is .............. and the cation $\mathrm{M^{2+}(aq)}$ is ..............
\begin{itemize}
\item[(1)] $-0/4$, reducer \quad (2) $+0/4$, oxidizer \quad (3) $-0/76$, reducer \quad (4) $-0/76$, oxidizer
\end{itemize}
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