- Acid dissociation – (expressed quantitatively) acid dissociation constant, Ka, is nothing more than the equilibrium constant for the dissociation reaction of an acid in water.
Relative strength of an acid ↑ (increases), its Ka ↑ (increases) and its pKa ↓(decreases).
(The Ka and pKa of an acid depend on the strength of an acid, but not its concentration.) - Base hydrolysis – base hydrolysis constant, Kb, nothing more than the equilibrium constant for the hydrolysis reaction of a base in water.
Relative strength of a base ↑ (increases), its Kb ↑ (increases) and its pKb ↓ (decreases).
(The Kb and pKb of an acid depend on the strength of an acid, but not its concentration.) - Overall Relationship : Acid strength ↑ , Ka ↑ , pKa ↓ , conjugate base strength ↓, Kb ↓, pKb ↑
- Strength of a reagent (Ka / pKa and Kb / pKb) – the completeness of a reaction in water. (dissociation = ionisation or electrolytic nature)
The stronger the acid, the more electrolytic it is, because it conducts electricity better due to the greater number of ions in solution.
The stronger the base, the more readily it undergoes hydrolysis when mixed with water
| Acid | Name | pKa |
| Cl3CCOOH | Trichloroacetic acid | 0.64 |
| Cl2HCCOOH | Dichloroacetic acid | 1.27 |
| H2SO3 | Sulfurous acid | 1.82 |
| HClO2 | Chloroacetic acid | 1.90 |
| ClH2CCOOH | Chloroacetic acid | 2.82 |
| HF | Hydrofluoric acid | 3.15 |
| HNO2 | Nitrous acid | 3.41 |
| HCOOH | Formic acid | 3.74 |
| H3CCOOH | Acetic acid | 4.74 |
| 2,4-(H3C)2C6H3NH3+ | 2,4-dimethylanilinium | 5.08 |
| 4-H2NC6H4NH3+ | 4-aminoanilinium | 6.18 |
| H3CO3 | Carbonic acid | 6.36 |
| 4-O2NC6H4OH | 4-nitrophenol | 7.15 |
| HClO | Hypochlorous acid | 7.46 |
| HBrO | Hypobromous acid | 8.72 |
| NH4+ | Ammonium | 9.26 |
| HCN | Hydrogen cyanide | 9.36 |
| HIO | Hypoiodous acid | 10.66 |
