Acid
A substance that donates a proton in solution, forming hydronium
Base
A substance that accepts a proton in solution, forming hydroxide
Strong acid
An acid that fully dissociates into ions in solution
Strong base
A base that fully dissociates into ions in solution
Weak acid
An acid that only partially dissolves into ions in solution
Weak base
A base that only partially dissolves into ions in solution
Equilibrium
When a reaction does not go to completion, rate of forward and backward reactions are equal
Solubility
The measure of how much substance dissolves
Solubility constant
Ks
Alkali
A base that is soluble
pH
Measure of the acidity or alkalinity of a solution
Hydronium
ions, formed from an acid in solution
Hydroxide
ions, formed from a base in solution
Salt
Formed when an acid and base react
Ionic product
The product of the concentrations of ions present
Precipitate
An insoluble solid suspended in solution
A precipitate forms when…
IP>Ks
Common ion effect
Solubility decreases when a common ion is present
Hydrobromic acid
, a strong acid
Hydrochloric acid
, a strong acid
Nitric acid
, a strong acid
Sulphuric acid
, a strong acid
Ethanoic acid
, a weak acid
Hydrofluoric acid
, a weak acid
Ammonium
, a weak acid
Potassium hydroxide
, a strong base
Sodium hydroxide
, a strong base
Ammonia
, a weak base
Ethanoate
, a weak base
Methylamine
, a weak base
Solvent
The substance that dissolves the solute
Solute
The substance that is dissolved in the solvent
Sparingly soluble
Very little of the substance dissolves
Equilibrium constant
Kc
Monoprotic
A substance that can only donate or accept one proton
Diprotic
A substance that can accept or donate two protons
Amphiprotic
A substance that can either donate or accept protons
Conjugate acid
Formed when a base donates a proton
Conjugate base
Formed when an acid accepts a proton
Conductivity
A measure of how strongly a substance can conduct electricity. Free ions or electrons must be present in order to conduct electricity
Electrolyte
Solution that contains ions and can conduct electricity
Acidity constant
Ka
Base constant
Kb
Ionic product of water
Kw
Relationship between Ka and Kb
Kw = Ka x Kb
Titration
Gradual addition of a substance of known concentration to a substance of unknown concentration to determine concentration
Titration curve
Plot of pH versus volume as a titration takes place
Equivalence point
Point where equivalent amounts of solutions have been added. In strong acid/strong base titrations, the base and acid would neutralise at the equivalence point
Buffer zone
Region where pH remains constant
Buffer solution
Substance that resists changes in pH
Acid salt
A salt that donates a proton to form hydronium ions in solution
Base salt
A salt that accepts a proton, forming hydroxide in solution.
pKa=pH
[acid]=[base]
pKa>pH
[acid]<[base]
pKa<pH
[acid]>[base]