Editing Conjugate (acid-base theory) (section)

==Table of acids and their conjugate bases==
Below are several examples of acids and their corresponding conjugate bases; note how they differ by just one proton (H<sup>+</sup> ion). Acid strength decreases and conjugate base strength increases down the table.

{| class="wikitable"
|-
! Acid
! Conjugate base
|-
| {{Chem|H|2|F|+}} [[Fluoronium]] ion
| HF [[Hydrogen fluoride]]
|-
| HCl [[Hydrochloric acid]]
| Cl<sup>−</sup> [[Chloride]] ion
|-
| H<sub>2</sub>SO<sub>4</sub> [[Sulfuric acid]]
| HSO{{su|b=4|p=−}} [[Hydrogen sulfate]] ion (''bisulfate'' ion)
|-
| HNO<sub>3</sub> [[Nitric acid]]
| NO{{su|b=3|p=−}} [[Nitrate]] ion
|-
| H<sub>3</sub>O<sup>+</sup> [[Hydronium]] ion
| H<sub>2</sub>O [[water (molecule)|Water]]
|-
| HSO{{su|b=4|p=−}} [[Hydrogen sulfate]] ion
| SO{{su|b=4|p=2−}} [[Sulfate]] ion
|-
| H<sub>3</sub>PO<sub>4</sub> [[Phosphoric acid]]
| H<sub>2</sub>PO{{su|b=4|p=−}} [[Dihydrogen phosphate]] ion
|-
| CH<sub>3</sub>COOH [[Acetic acid]]
| CH<sub>3</sub>COO<sup>−</sup> [[Acetate]] ion
|-
| HF [[Hydrofluoric acid]]
| F<sup>−</sup> [[Fluoride]] ion
|-
| H<sub>2</sub>CO<sub>3</sub> [[Carbonic acid]]
| HCO{{su|b=3|p=−}} [[Hydrogen carbonate]] ion
|-
| H<sub>2</sub>S [[Hydrosulfuric acid]]
| HS<sup>−</sup> [[Hydrosulfide]] ion
|-
| H<sub>2</sub>PO{{su|b=4|p=−}} [[Dihydrogen phosphate]] ion
| HPO{{su|b=4|p=2−}} [[Monohydrogen phosphate|Hydrogen phosphate]] ion
|-
| NH{{su|b=4|p=+}} [[Ammonium]] ion
| NH<sub>3</sub> [[Ammonia]]
|-
| H<sub>2</sub>O Water ([[pH]]=7)
| OH<sup>−</sup> [[Hydroxide]] ion
|-
| HCO{{su|b=3|p=−}} [[Hydrogencarbonate]] ''(bicarbonate)'' ion
| CO{{su|b=3|p=2−}} [[Carbonate]] ion
|}