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

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

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Answer 1 · 2015-11-19T16:01:52

$H_{3} C - C (= O) O H (a q) + H_{2} O ⇌ H_{3} C - C (= O) O^{-} (a q) + H_{3} O^{+}$ $H_3C-C(=O)OH(aq) +H_2O rightleftharpoons H_3C-C(=O)O^(-)(aq) +H_3O^+$

Explanation:

The conjugate base of acetic acid is the acetate anion (the parent acid less a proton, $H^{+}$ $H^+$ ), hence $H_{3} C - C (= O) O^{-}$ $H_3C-C(=O)O^(-)$ . The conjugate acid of $O H_{2}$ $OH_2$ is water plus a proton, i.e. an hydronium ion, $H_{3} O^{+}$ $H_3O^+$ . This is a representation, and as far as anyone knows the hydronium ion is a cluster of 3-4 water molecules (say $O_{3} H_{6}$ $O_3H_6$ ) plus a proton to give $H_{7} O_{3}^{+}$ $H_7O_3^+$ . To represent the reactivity of this species in aqueous solution, $H^{+}$ $H^+$ or $H_{3} O^{+}$ $H_3O^+$ , are entirely appropriate shorthands.

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

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