Hi,
I was thinking if you have a buffer solution say ethanoic acid and sodium ethanoate to produce:
CH3COOH <--> H+ + CH3COO-
and you increase the concentration of H+, i know equilibrium will shift to the left and so the CH3COO- will react with the H+ using up most of it. What i dont understand is why its only most, is it because the acid dissociation constant needs to be restored and both H+ and CH3COO- will decrease when they are reacting so H+ does not need to decrease to its intitial level?
Also, because H+ does not decrease to its intial level surely that implies that the concentration of OH- ions has reduced to keep the constant value of kw, but how does this happen if it does?
Thanks for your help