Properties of Acids and Bases

Ionisation Reaction

Ionisation Reaction

Reaction of acid with water

Monoprotic Acids

Acids that only give up 1 proton (example: HCl and HNO3)

Diprotic Acids

Acids that only give up 2 protons (example: H2SO4 and H2CO3)

Triprotic Acids

Acids that only give up 3 protons (example: H3PO4)

Hydrogens bonded to Carbons…

Hydrogens bonded to Carbons won’t dissociate to produce H+’s

Acids that nearly fully dissociate

Strong acids that produce lots of ions (example: HCl, H2SO4)

Acids that hardly dissociate

Weak acids that don’t produce many ions (example: acidic acid, citric acid)

Ka

acid dissociation constant

Kb

base dissociation constant

Large Ka value

Strong acids because acid is largely dissociated into its ions

Large Ka

Favours formation products

Small Ka value

Little acids dissociates therefore weak acids

Strong Acids

an acid that readily donates a proton to water (Large Ka)

Larger Kb value

strong base because it has a high level of dissociation

Large Kb

favours formation products

Small Ka value

little base dissociates therefore weak base

Weak acids

an acid in which only a small proportion of the molecules will donate their proton

Increase in concentration =

Increase in molarity

Decrease in concentration (dilute) =

Decrease in Molarity

Strength of strong acid or base

100% ionised in water, has strong electrolytes and has an high conductivity of electron flow

Strength of weak acid or base

Doesn’t ionise complete therefore has a weak electrolyte and poor conductors