Calculate the pH at which the following conversion (reaction) will be at equilibrium in basic medium ? `I_2(s)hArr I^(-)(aq)+IO_(3)^(-)(aq)` When the

Calculate the pH at which the following conversion (reaction) will be at equilibrium in basic medium ?
`I_2(s)hArr I^(-)(aq)+IO_(3)^(-)(aq)`
When the equilibrium concentrations at 300 K are `[I^(-)]` =0.10 M and `[IO_3^(-)]=0.10 M`
{Given that `DeltaG_f^@(I^(-)aq)`=-50 kJ/mole , `DeltaG_f^(@)(IO_3^(-),aq)`=-123.5 kJ/mole , `DeltaG_f^(@)(H_2O,l)=-233` kJ/mole , `DeltaG_f^(@)(OH^(-),aq)`=-150 kJ/mole , Ideal gas constant =R=`25/3` J `"mole"^(-1)K^(-1),log e =2.3 , `deltaG_f^@` (element, standard state )=0, `DeltaG_r^@`(reaction)`=sumv_pDeltaG_f^@`(products)- `sumv_rDeltaG_f^@`(reactants), where `v_p` and `v_r` are the stochiometric coefficients in the balanced chemiclal equation. }