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Summary of Chapter 8 of the Chemistry for the IB Diploma Coursebook
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8 ACIDS AND BASES8.1 THEORIES OF ACIDS AND BASES
ACIDS BASES
Characteristics: Characteristics :
Corrosive Cleaning agents
Hydrogen Detergents
Sour taste Caustic / Corrosive
o citric acid- lemon Slippery / soap
Examples :
- Bases : Oxides, NaOH
- Acids : HCl, NO3
BRØNSTED–LOWRY ACIDS AND BASES
The Brønsted–Lowry definition is:
an acid is a proton (H+) donor
a base/alkali is a proton (H+) acceptor
Ethanoic acid + Water ⇋ Ethanoate + Hydronium ION
Acid Base Base Acid
CONJUGATE ACID–BASE PAIRS ALWAYS DIFFER BY ONE PROTON (H+).
, AMPHIPROTIC AND AMPHOTERIC
Amphiprotic refers to species that can donate (acting as an acid) or accept (acting as a base) a
proton
Amphoteric is a more general term and refers to a substance that can act as an acid and a base
8.2 LEWIS ACIDS AND BASES (HL)
Lewis definition :
An acid is an electron pair acceptor.
A base is an electron pair donor.
A COORDINATE (DATIVE) COVALENT BOND IS ALWAYS FORMED IN A LEWIS ACID–BASE REACTION.
For a substance to act as a Lewis base, it must have a lone pair of electrons. For a substance to act
as a Lewis acid, it must have space to accept a pair of electrons in its outer shell
8.3 PROPERTIES OF ACIDS AND BASES
REACTION OF ACIDS AND BASES
ACIDS WITH METAL
Metal + Acid → Salt + Hydrogen
Unreactive metals such as copper do not react with dilute acids.
ACIDS WITH CARBONATES AND HYDROGENCARBONATES
Acid + Carbonate / Hydrogencarbonate → Salt + Carbon dioxide + Water
ACIDS WITH BASES AND ALKALIS
Base / Alkali + Acid → Salt + Water
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