Cathodic reaction : $2{H^ + } \to {H_2}({P_2})$
${E_{cathode}} = - \frac{{RT}}{{2F}}\ln \frac{{{P_2}}}{{{{[{H^ + }]}^2}}}$ ;${E_{{\rm{anode}}}} = - \frac{{RT}}{{2F}}\ln \frac{{{{[{H^ + }]}^2}}}{{{P_1}}}$
${E_{\inf }} = {E_{anode}} + {E_{cathode}}$$ = - \frac{{RT}}{{2F}}\ln \frac{{{{({H^ + })}^2}}}{{{P_1}}} - \frac{{RT}}{{2F}}\ln \frac{{{P_2}}}{{{{({H^ + })}^2}}}$
$= - \frac{{RT}}{{2F}}\ln \frac{{{P_2}}}{{{P_1}}} = \frac{{RT}}{{2F}}\ln \frac{{{P_1}}}{{{P_2}}}$.
(નજીકના પૂર્ણાંકમાં રાઉન્ડ ઑફ કરો) $[$ આપેલ $\left.: \frac{2.303 RT }{ F }=0.059\right]$
$H_3PO_4 + OH^- \rightarrow H_2PO_4^- + H_2O$ ;
$H_3PO_4 + 2OH^- \rightarrow HPO_4^{2-} + 2H_2O$ ;
$H_3PO_4 + 3OH^- \rightarrow PO_4^{3-} + 3H_2O$