Acid-base: comparative table

151 0 0 25 March, 2022

Table to compare acid-base theories.

The following table shows the different acid-base theories:

Acid-base theory	Definition of acid	Example of acid	Definition of base	Example of base
Arrhenius	A species that increases the concentration of hydrogen ions, H⁺, in an aqueous solution. The H⁺ ions react immediately with the H₂O to form oxidanium ions (H₃O⁺).	HCl_(ac)→H+_(ac)+Cl-_(ac)	A species that increases the concentration of hydroxide ions, OH-, in an aqueous solution.	NaOH_(ac)→Na+_(ac)→OH ^– _(ac)
Brønsted-Lowry	Proton-donating species, H⁺. Water is defined as an amphoteric substance since it can act as an acid or a base. Conjugated acid is the species formed when a Brønsted-Lowry base accepts a proton.	NH3(g)+HCl(g) →NH4Cl(s) * It is also expressed as * Conjugated acid	A species that accepts a proton, which requires a lone pair of electrons to bond to H+. *Conjugate base is the species formed after a Brønsted-Lowry acid gives up a proton.	NH3(ac)+H2O(l⇌NH4+(ac)+OH-(ac) Conjugate base OH-(ac*)
Lewis	Species that accepts and shares a pair of electrons yielded by a base.	Acid + Base → adduct H++ :NH3	A species that gives up a pair of electrons and shares them with an acid.	Acid + Base → adduct

Reaction	Arrhenius	Brønsted-Lowry	Lewis	Comment
HCl + NaOH → NaCl +_H2O	Acid + Base → Salt + Water HCl + NaOH → NaCl +_H2O	Acid + Base → Base conj. + Acid conj. HCl + NaOH → NaCl + _H2O	Acid + Base → adduct HCl + NaOH → NaCl +_H2O
_H2PO4-+ HCl → H3PO4 + Cl-	Not applicable	Acid + Base → Acid conj. + Base conj. _H2PO4- + HCl → H3PO4 + Cl-	Acid + Base → adduct _H2PO4- + HCl → H3PO4 + Cl-	* The Arrhenius theory does not apply because an OH ion is necessary for the definition.
AlCl3 + NH3 → [Al(NH3)Cl3].	Not Applicable	Not applicable	Acid + Base → adduct AlCl3 + NH3 → [Al(NH3)Cl3].	* All Brønsted-Lowry acids and bases are Lewis acids and bases, but not all Lewis acids and bases are Brønsted-Lowry acids and bases.