· Corrosive liquids
· Have a sour taste
· Give characteristic colors with indicators
Acids also were known to react with:
· Bases (and alkali) to give a salt and water – neutralization reaction
· Carbonates to give salt, carbon dioxide (observed as effervescence) and water
· Some metals to give a salt and hydrogen
Ideas have developed about acids and acidity:
The theory of electrolytic dissociation: it states that when acids, bases or salts dissolve in water they split up partially or completely into their ions.
· Arrhenius acids give hydrogen ions in aqueous solution
HA (aq) ⇌ H+ (aq) + A- (aq)
· Arrhenius bases give hydroxide ions in aqueous solution
BA (aq) + H2O (aq) ⇌ BH+ (aq) + OH- (aq)
Limitations of the theory: some acid-base reaction took place in solvents other than water or did not even need water to react. The theory restricts reactions to aqueous solutions only.
The theory proposed that:
· An acid is a proton (H+) donor
· A base is a proton acceptor
· Acid-base Equilibria involve the transfer of protons
· Each acid has a conjugate base
· Each base has a conjugate acid
HA (aq) + H2O (l) ⇌ H3O+ (aq) + A- (aq)
The acid HA is transformed into A- after donating a proton to the base, H2O. In the reverse reaction, the A- ion acts as a base by accepting a proton to form the acid again. Therefore, HA and A- are referred to as conjugate acid-base pairs. Similarly, H2O and H3O+ are conjugate acid-base pairs.