15 Acid-Base Equilibria Flashcards
(12 cards)
Strong Acid/ Base
Definition
An acid/ base that undergoes complete dissociation in aqueous medium to produce H+/ OH-(aq).
Weak Acid/ Base
Definition
An acid/ base that undergoes partial dissociation in aqueous medium to produce H+/ OH-(aq).
Concentration
Definition
The amount of acid per unit volume of the solution.
Basicity of an Acid
Definition
ie. Proticity
The number of H atoms that can be ionised to H+ per molecule of acid.
Arrhenius Theory of Acids & Bases
Definition
Acid: Releases H+(aq)
Base: Releases OH-(aq)
Arrhenius Theory of Acid & Bases
Limitations
- Restricts acid-base reactions to those that occur in (aq)
- Did not acocunt for the basic properties of NH3 and other substances such as amines that do not contain the -OH group
- Focuses on the existence of the H+ ion in (aq) but in reality H+ does not exist
Hydronium Ion
Equation
ie. Hydroxonium Ion/ Hydrated Proton
H2O (I) + H+ (aq) –> H3O+ (aq)
via Dative Covalent Bond
Bronsted-Lowry (BL) Theory of Acid & Bases
Definition
BL Acid: H+ Donor
BL Base: H+ Acceptor
Bronsted-Lowry (BL) Theory of Acid & Bases
Acid-Base Reaction
Transfer of a proton ie. H+ from acid to base
Acid is an acid in the presence of a base and vice versa
Bronsted-Lowry (BL) Theory of Acid & Bases
Key Example, H2O which is Amphiprotic
Donation & acceptance of H+ is possible
–> Enables H2O to be both an acid & a base
Eg. Nitration of Benzene
H2S04 + HNO3 –> H2NO3+ + HSO4-
Lewis Acids & Bases
Definition
Acid: a species that can accept a pair of electrons from a base to form a Dative Covalent bond ie. e-pair acceptor
Base: a species that can donate a pair of electrons from an acid to form a Dative Covalent bond ie. e- pair donor
Conjugate Acid-Base (CAB) pair
Definition
