Acids and bases

What is an amphoteric compound

A compound that can act as both a base and an acid, donating and accepting protons

What is an electrolyte?

A molecule that will form ions when it dissociates in a suitable solvent

Describe dissociation of acids

• Acids give away protons

• Dissociation of strong acids have reactions that aren’t reversible

• Dissociation of weak acids have reactions that are reversible

Describe dissociation of bases

• Bases accept protons

• Dissociation of strong bases have reactions that aren’t reversible

• Dissociation of weak bases have reactions that are reversible

What is a monovalent, divalent and trivalent compound

Compounds with a charge of 1, 2 and 3

What is a Normal (N)?

• A unit of concentration. It is the number of equivalent(s) (Eq) in 1L of solution

• N = M × Valence

Describe strong electrolytes

Dissociation is almost complete and they exist almost fully as ions in solution

Describe weak electrolytes

Dissociation is incomplete and they exist as a mixture of unionised and ionised species

What is the equation linking pH and H₃O⁺?

• pH = -log[H₃O⁺]

• H₃O⁺ = 10^-pH

What is the acidity constant?

What is the Henderson-Hasselbach equation

What is the equation for the concentration of a weak acid in a solution?

What is the equation for the degree of ionisation of a weak acid?

Here 'charge' for a weak acid is -1. Whilst charge for a weak base is +1