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Conjugate acid
In the Brønsted-Lowry (protonic) theory of acids and bases, a conjugate acid is the acid member, HX, of a pair of two compounds that transform into each other by gain or loss of a proton. The base produced, X-, is called the conjugate base. In aqueous solution, the chemical reaction involved is of the form
- HX + H2O ↔ X- + H3O+
This principle is discussed in detail in the article on acid-base reaction theories.
Tabulated below are several examples of conjugate acid-base pairs. Acid strength decreases and base strength increases down the table. (The dissociation reaction reaches equilibrium further to the right, with more X- produced.)
| Acid | Base |
|---|---|
| HCl Hydrochloric acid | Cl- Chloride ion |
| H2SO4 Sulfuric acid | HSO4- Hydrogen sulfate ion |
| HNO3 Nitric acid | NO3- Nitrate ion |
| H3O+ Hydronium ion | H2O Water |
| HSO4- Hydrogensulfate ion | SO42- Sulfate ion |
| H3PO4 Phosphoric acid | H2PO4- Dihydrogen phosphate ion |
| HC2H3O2 Acetic acid | C2H3O2- Acetate ion |
| H2CO3 Carbonic acid | HCO3- Hydrogen carbonate ion |
| H2S Hydrosulfuric acid | HS- Hydrogen sulfide ion |
| H2PO4- Dihydrogen phosphate ion | HPO4+ Hydrogen phosphate ion |
| NH4+ Ammonium ion | NH3 Ammonia |
| HCO3- Hydrogen carbonate ion | CO32- Carbonate ion |
| HPO42- Hydrogen phosphate ion | PO43- Phosphate ion |
| H2O Water | OH- Hydroxide ion |
03-10-2013 05:06:04
The contents of this article is licensed from www.wikipedia.org under the GNU Free Documentation License. Click here to see the transparent copy and copyright details
The contents of this article is licensed from www.wikipedia.org under the GNU Free Documentation License. Click here to see the transparent copy and copyright details