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.

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