Reactivity 3.1- Proton Transfer Reactions
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What is the Bronsted-Lowry acid-base theory.
It defines acids and bases by their ability to donate/accept electrons.
Bronsted-Lowry Acid
Proton donor
Bronsted-Lowry Base
Proton acceptor
Amphiprotic
Can both donate and accept protons
Amphoteric
Can act as either an acid or base (not all amphoteric substances are amphiprotic)
Hydronium ions
H3O+, formed in water as in aqueous solutions protons do not exist freely, instead they combine with water molecules
Conjugate base
When a BL acid loses a proton
Conjugate acid
When a BL base gains a proton
Are all alkali’s bases?
yes
Alkali’s
Bases that dissolve in water to produce OH-
How is the strength of an acid/base determined?
By it’s degree of ionisation in solution
pH scale
A measure of the H+ concentration in solution expressed in logarithmic form
What is a pH of 7
Neutral
pH<7
Acidic
pH>7
Basic
What change in H+ will there be for a change of 1pH unit
Tenfold change in H+ ion concentration
What is pure water slightly dissociated into?
H+ and OH-
What is Kw
The ionic product constant for water.
____ acids and bases are completely dissociated in solution.
Strong
____ acids and bases are partially dissociated in solution.
Weak
Ka
acid dissociation constant
Kb
base dissociation constant
Property of strong acids and bases due to their high level of ionisation.
High electrical conductivity
What is different about a rxn with a weak acid rather than a strong one?
The rate of rxn is lower