Grade 12 Chemistry - Bronsted Lowry Acid & Base - Reaction of Acid or Base with Water - Amphiprotic

Bronsted-Lowry acid is a hydrogen ion donor
Bronsted-Lowry acid is a H+ donor
Bronsted-Lowry base is a hydrogen ion acceptor
Bronsted-Lowry base is a H+ acceptor
Strong acid or base - dissociates completely into ions (strong electrolyte)
Weak acid or base - does not dissociate completely into ions (weak electrolyte)
Amine (NH2) is a base because it has nitrogen atom with at least one lone electron pair that has the tendency to accept a hydrogen ion
Amine (NH2) is a base because it has nitrogen atom with at least one lone electron pair that has the tendency to accept a H+
Carboxylic acid group (COOH) has a hydrogen ion that can be donated
Carboxylic acid group (COOH) has a H+ that can be donated
Water acts as base when an acid is added
Water acts as acid when an base is added
Water can act as acid or base
Water is amphiprotic
A substance is amphiprotic if it can donate or accept a hydrogen ion
A substance is amphiprotic if it can donate or accept a H+
How to write the chemical equation for reaction of acid or base with water
Writing the chemical equation for reaction of acid or base with water

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A substance is amphiprotic when it can donate or accept a hydrogen ion