A weak acid or a weak base only partially dissociates. At equilibrium, both the acid and the conjugate base are present in solution
Weak acid: AH + H2O ↔ A-(aq) + H3O+(aq)
Weak base: BOH + H2O ↔ B+(aq) + OH-(aq) or
B + H2O ↔ BH+(aq) + OH-(aq)
Examples of weak acids and bases are given in the table below.
Stronger acids have a larger acid dissociation constant (Ka) and a smaller logarithmic constant (pKa = −log Ka) than weaker acids. The stronger an acid is, the more easily it loses a proton, H+.
Two key factors that contribute to the ease of deprotonation are the polarity of the H—A bond and the size of atom A, which determines the strength of the H—A bond. Acid strengths also depend on the stability of the conjugate base.
See also Acid-base properties of aqueous solutions of salts with ions from both acids and bases, Buffer solutions, pKa of inorganic acids and bases, pKa of phenols, alcohols and carboxylic acids and pKa of amines, diamines and cyclic organic nitrogen compounds, as well as Acid and base pH indicators or pH values of some solutions of acids and bases.
|Stong Acids ||Strong Bases|
|Hydrobromic acid||HBr||Barium hydroxide||Ba(OH)2|
|Hydrochloric acid||HCl||Calsium hydroxide||Ca(OH)2|
|Hydroiodic acid||HI||Lithium hydroxide||LiOH|
|Nitric acid||HNO3||Potassium hydroxide||KOH|
|Perchloric acid||HClO4||Sodium hydroxide||NaOH|
|Sulfuric acid||H2SO4||Strontium hydroxide||Sr(OH)2|
|Weak acids || Weak bases |
|Hydrocyanic acid||HCN||Sodium bicarbonate||NaHCO3|
Material properties of gases, fluids and solids - densities, specific heats, viscosities and more.
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