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. }

Calculate the pH at which the following conversion (reaction) will be

1.	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. }
Answer» SOLUTION :Balanced equation will be `3I_2(s)+6OH^(-)hArr5I^(-)(AQ)+IO_(3)^(-)(aq)+3H_2O(l)` `DeltaG^(@)=-172.5 "kJmole"^(-1)=-25/3xx300xx2.3xx10^(-3)`log k log k=30 `10^(30)=(10xx^(-5)xx10^(-1))/([OH^(-)]^(6))` so `[OH^-]=10^(-6)` and therefore `[H^+]=10^(-8)` so, pH=8