Now that we’ve defined acids and bases, let’s discuss how they work together in reactions. Look at the generic acid-base reaction below:
HX(aq) + H2O(l) 
X-(aq) + H3O(aq)
When the forward reaction occurs, HX donates a proton to water (so it acts as the base) to form hydronium. When the reverse reaction occurs, the hydronium ion acts as the acid, donating a proton to the X-. Together, HX and X- are said to be conjugate acid-base pairs. Conjugate acid-base pairs are compounds that differ by the presence of one proton, or H+. All acids have a conjugate base, which is formed when their proton has been donated; likewise, all bases have a conjugate acid, formed after they have accepted a proton.
Example
Apply the appropriate acid-base theory to first identify the acid and base reacting and then identify the conjugate acid-base pairs in the examples below:
Explanation
- In this first reaction, we see that HNO3 gives a proton to water, which then forms a hydronium ion. This makes HNO3 the acid in the forward reaction, and water acts as the base. HNO3’s conjugate base is
, and water’s conjugate acid is the hydronium ion, or 
- Here
donates the proton to water, so in the forward reaction it acts as the acid, and water is still the base. 
’s conjugate base is NH3, and water’s conjugate acid is again the hydronium ion, H3O+.
Relative Strengths of Acids and Bases
Certain acids are stronger than other acids, and some bases are stronger than others. What this means is that some acids are better at donating a proton, and some bases are better proton acceptors. A strong acid or base dissociates or ionizes completely in aqueous solution. A weak acid or base does not completely ionize.
Strong Acids
There are six strong acids that you’ll need to memorize for the SAT II Chemistry test:
- Hydrohalic acids: HCl, HBr, HI
- Nitric acid: HNO3
- Sulfuric acid: H2SO4
- Perchloric acid: HClO4
Let’s take a closer look at how acids differ in strength by focusing on perchloric acid. In general, the greater the number of oxygen atoms in a polyatomic ion, the stronger the acid.
So HClO4 is stronger than HClO3, which is stronger than HClO2, which is stronger than HClO. (Perchloric acid is the strongest among the six, but all the other oxyacids of chlorine are not considered strong acids.) Now think about why, as you take away oxygens, the strength of the acid decreases. The hydrogen (proton) to be removed is bonded to an oxygen atom. The oxygens are highly electronegative and are pulling the bonded pair of electrons away from the site where the hydrogen is bonded, thus making it easier to remove the H+. As the number of oxygen decreases, the molecule becomes less polar, and the H+ is harder to remove.
Strong Bases
There are fewer strong bases to memorize for the exam. These are hydroxides (—OH), oxides of 1A and 2A metals (except Mg and Be), H
-, and
. Remember that the stronger the acid, the weaker its conjugate base, and the converse is also true. The figure below illustrates the relative strengths of some common conjugate acid-base pairs.
