Chemistry - Electrochemistry Question with Solution | TestHub

Calculate the pH at which the following reaction will be at equilibrium in basic medium:

${\mathrm{Br}}_2(\mathrm{l})\to {\mathrm{Br}}^{-}(\mathrm{aq})+{\mathrm{BrO}}_3^{-}(\mathrm{aq})$ (to be balanced)

when the equilibrium concentrations at 300 K are $\left[{\mathrm{Br}}^{-}\right]=0.1$ M and $\left[{\mathrm{BrO}}_3^{-}\right]=0.1$ M.

Given $\Delta G_f^{\circ }$ of ${\mathrm{OH}}^{-}(\mathrm{aq})=-160$ kJ/mol, of ${\mathrm{H}}_2\mathrm{O}(\mathrm{l})=-240$ kJ/mol, of ${\mathrm{Br}}^{-}(\mathrm{aq})=-70$ kJ/mol, of ${\mathrm{BrO}}_3^{-}(\mathrm{aq})=-28$ kJ/mol; $R=\frac{25}{3}$ J/mol/K, $\ln 10=2.3$.