acid-base equilibrium

universal indicator pH

below 7 is acidic, above 7 is basic and 7 is neutral

neutralisation

reaction of an acid and base to form salt and water

acid

proton or hydrogen ion donor

base

proton or hydrogen ion acceptor

salt 

formed when an acid reacts with alkali, metal oxide or metal carbonate 

alkalis

bases that are soluble in water

Bronsted lowry acid

proton (H+) donor

Bronsted lowry base

proton (H+) acceptor

amphoteric 

ability to act as both acids and bases 

forward arrow —>

reaction goes to completion

equilibrium arrow ←—>

reaction doesnt go into completion

degree of dissociation

extent to which a molecule of an acid ionises in a solvent to form H+ ions or a base forms OH- ions

strong acids and bases 

dissociate completely in solution 

weak acids and bases

partially dissociate in solution

pH values of strong vs weak acids

strong acids have a lower pH in the same concentration due to a higher concentration of H+ ions

electrical conductivity of strong vs weak acids

strong acids have great conductivity due increased concentration of H+ ions

acid-base indicator 

compound that shows colour change based on solution being acidic, basic or neutral

strong acids and strong bases

sharp fall in pH

strong acids and weak bases

weak acids and strong bases

weak acids and bases