For the auto-ionization of water at `25^(@)C, H_(2)O(l)iff H^(+)(aq)+OH^(-)` (aq) equilibrium constant is `10^(-14)`.
What is `DeltaG^(@)` for the process?

To calculate K_(W) of water H_(2)O(l)+H_(2)O_(l)toH_(2)O^(+)(aq)+OH^(-)(aq)

The equilibrium constant for the ionization of RNH_(2) (g) in water as RNH_(2)(g)+H_(2)O(l)hArrRNH_(3)^(+)(aq)+OH^(-)(aq) is 8xx10^(-6) at 25^(@)C. find the pH of a solution at equilibrium when pressure of RNH_(2) (g) is 0.5 bar :

The equilibrium constant for the ionization of RNH_(2) (g) in water as RNH_(2)(g)+H_(2)O(l)hArrRNH_(3)^(+)(aq)+OH^(-)(aq) is 8xx10^(-6) at 25^(@)C. find the pH of a solution at equilibrium when pressure of RNH_(2) (g) is 0.5 bar :

The equilibrium constant for the ionisation of RNH_(2(g)) in water as RNH_(2(g)) + H_(2)O_((l)) hArr "RNH"_(3(aq))^(+) + OH_((aq))^(-) is 8 xx 10^(-6) at 25^(@) C . Find the pH of a solution at equilibrium when pressure of RNH_(2(g)) is 0.5 bar.

For the equilibrium (autoprotolysis of water), 2H_(2)O iff H_(3)O^(+)+OH^(-) , the value of DeltaG^(0) at 298 K is approximately?