Bronsted-lowery Acids and Bases
Conjugate Acid-Base Pairs
HX(aq) + H2O(l) <-----> X-(aq) + H3O+(aq)in any acid-base equilibrium both the forward reaction (to the right), and the reverse reaction (to the left), involve proton transfer.
forward reaction HX donates a proton to H2O, so HX is the Bronsted-lowry acid., and H2O is the Bronsted-lowry base.
in the reverse reaction, the H3O+ ion donates a proton to the X- ion, so H3O+ is the acid and X- is the base.
when the acid HX donates a proton, it leaves behind a substance, X- which can act as a base, when H2O acts as a base, it generates H3O+ is the acid, and X- is the base.
when the acid HX donates a proton, it leaves behind a substance, X_ which can act as a base, when H2O acts as a base, it generates H3O+, which can act as an acid.
Conjugate acid-base pair is an acid and a base such as HXand X- that differ only in the presence or absence of a proton.
Conjugate base of the acid is every acid formed by removing a proton from the acid.
example, OH- is the conjugate base of H2.
X- is the conjugate base of HX.
conjugate acid of the base, is every base formed by adding a proton to the base.
H3O+ is the conjugate acid of H2O.
HX is the conjugate acid of X-