I would like to ask a question about thermodynamics which we covered in
the biochemistry lessons. D Go = - R T ln K
If for example you take into consideration ethanoic acid <----->ethanoate
+ H+
and equilibrium constant for ethanoic acid is 1.7 x 10^-5.
By the equation:
D Go = - R T ln K (I used D instead of the letter delta)

Go would have a positive value. Therefore if you start with 1 mole pure
ethanoic acid and delta G is positive, I cannot understand why some
ethanoic acid dissociates on adding water to it.

My second point is why do we take delta G' as zero at equilibrium while we
don't take Delta Go'as zero? Both describe the equilibrium and at
equilibrium the net formation of energy is zero.