We should start by appreciating that in reality many acid-base reactions are equilibrium reactions, even if it doesn’t appear obvious at first sight.
In the case of hydrochloric acid:
But with ethanoic acid:
If the ethanoate ion, CH3COO–, will readily accept a proton from H3O+ to complete the back reaction, it is behaving as a base. We can say that the ethanoate ion is the conjugate base of ethanoic acid and that together, they make a conjugate acid-base pair.
Water of course is behaving as a base in accepting a proton from ethanoic acid in the forward reaction but in the back reaction, H3O+ is behaving as an acid in donating a proton to the ethanoate ion. H3O+ is the conjugate acid to water’s base. Another conjugate acid-base pair.
Let’s look at another example.
It is really important to appreciate that we are describing the behaviour of a substance in the context of a particular reaction (as defined by the equation), we are not giving substances labels. The HSO3– ion can also be seen behaving as a base:
Practice questions
- Identify the conjugate pairs in each of these reactions
(a) NH3 (aq) + H2O (l) ⇌ NH4+ (aq) + OH– (aq)
(b) HNO3 (aq) + OH– (aq) ⇌ NO3– (aq) + H2O (l)
(c) H2O (l) + H2O (l) ⇌ H3O+ (aq) + OH– (aq)
(d) HSO3– (aq) + H2O (l) ⇌ SO32- (aq) + H3O+ (aq)
2. Write an equation to show each of the following behaving as a base in solution – the product of the reaction will be the conjugate acid.
(a) OH– (aq) (b) HSO3– (aq) (c) CO3 2- (aq) (d) HCO3– (aq)
3. Write an equation to show the following behaving as an acid in solution – the product of the reaction will be the conjugate base.
(a) HCO2H (aq) (b) H2O (l) (c) HCO3– (aq) (d) H2S (aq)
- When ethanoic acid (CH3COOH) is added to the stronger fluoroethanoic acid (FCH2COOH) the mixture establishes an equilibrium. Write an equation for the reaction and identify the two conjugate acid-base pairs.
Answers
- (a) Base NH3 (aq) / Conjugate acid NH4+ (aq) ; Acid H2O (l) / Conjugate base OH– (aq)
(b) Base OH– (aq) / Conjugate acid H2O (l) ; Acid HNO3 (aq) / Conjugate base NO3– (aq)
(c) Base H2O (l) / Conjugate acid H3O+ (aq) ; Acid H2O (l) / Conjugate base OH– (aq)
(d) Base H2O (l)/ Conjugate acid H3O+ (aq) ; Acid HSO3– (aq) / Conjugate base SO32- (aq)
2. (a) OH– (aq) + H+ (aq) ⇌ H2O (l)
(b) HCO3– (aq) + H+ (aq) ⇌ H2SO4 (aq)
(c) CO3 2-(aq) + H+ (aq) ⇌ HCO3– (aq)
(d) HCO3– (aq) + H+ (aq) ⇌ H2CO3 (aq)
3. (a) HCO2H (aq) ⇌ H+ (aq) + HCO2– (aq)
(b) H2O (l) ⇌ H+ (aq) + OH– (aq)
(c) HCO3– (aq) ⇌ H+ (aq) + CO3 2–(aq)
(d) H2S (aq) ⇌ H+ (aq) + HS– (aq)
4. The stronger the acid, fluroroethanoic acid, will donate the proton to the weaker acid, ethanoic acid.
CH3COOH(aq) + FCH2COOH(aq) ⇌ CH3COOH2+(aq) + FCH2COO–(aq)