2.1.4: Acids Flashcards
Weak acid:
- Partially dissociates
* e.g. CH₃COOH ⇌CH₃COO⁻ + H⁺
Strong acid:
- Fully dissociates
* e.g. HCl ⟶ H⁺ + Cl⁻
Bronsted-Lowry base
A proton acceptor
Bronsted-Lowry acid
A proton (H⁺) donor
What is a monoprotic acid?
Donates 1 proton
Typical properties of acids
- Usually taste sour
- pH less than 7
- Aqueous solutions of acids contain H⁺ ions
- Acid = proton (H⁺) donor
Ionic equation for neutralisation reaction
H⁺ + OH⁻ ⟶ H₂O
Acid + base
Acid + base ⟶ salt + water
Acid + carbonate
Acid + carbonate ⟶ salt + water + carbon dioxide
Acid + metal
Acid + metal ⟶ salt + hydrogen
Acid + metal oxide
Acid + metal oxide ⟶ salt + water
Acid + metal hydroxide
Acid + metal hydroxide ⟶ salt + water
Conjugate base
The base that accepts the proton donated by the acid.
e.g. Cl⁻ in HCl
Concentrated acid
Fewer water molecules per unit volume than a dilute acid.
Acids release __ ions into solution
H⁺
Alkalis release __ ions into solution
OH⁻
Alkali
A soluble base
Salt
An ionic compound
How is a salt formed?
By replacing the H⁺ ions in an acid with metal ions.
Hydrated salts
Contain water molecules in their crystal structure
Given as .xH₂O
Anhydrous
Opposite of hydrated; salts that do not contain water molecules in their crystal structure.
What is the water in a hydrated salt known as?
Water of crystallisation
Molecules that can either donate or accept a proton depending on the circumstances
‘Amphiprotic’
Amphiprotic
Molecules that can either donate or accept a proton depending on the circumstances
