How would you identify the conjugate acid-base pairs in the equilibrium equation: HC2H3O2 + H2O --> H3O^+ + C2H3O2^-?

1 Answer
anor277
Nov 19, 2015

#H_3C-C(=O)OH(aq) +H_2O rightleftharpoons H_3C-C(=O)O^(-)(aq) +H_3O^+#

Explanation:

The conjugate base of acetic acid is the acetate anion (the parent acid less a proton, #H^+#), hence #H_3C-C(=O)O^(-)#. The conjugate acid of #OH_2# is water plus a proton, i.e. an hydronium ion, #H_3O^+#. This is a representation, and as far as anyone knows the hydronium ion is a cluster of 3-4 water molecules (say #O_3H_6#) plus a proton to give #H_7O_3^+#. To represent the reactivity of this species in aqueous solution, #H^+# or #H_3O^+#, are entirely appropriate shorthands.

Related questions
See all questions in Conjugate Acids and Conjugate Bases
Impact of this question
11151 views around the world
You can reuse this answer
Creative Commons License