Arrhenius Acid: A substance that yields hydrogen ions (H+) when dissolved in water.

Arrhenius Base: A substance that yields hydroxide ions (OH-) when dissolved in water.

Bronsted acid : A substance capable of donationg a proton.

Bronsted base: A substance capable of accepting a proton.

Chemical Equilibrium: A state in which the rates of the forward and reverse reactions are equal.

Chemical Reaction: A process in which a substance (or substances) is changed into one or more new substances.

End point: The volume of titrant required for the detection of the equivalence point.

Equilibrium constant: A number equal to the ratio of the equilibrium concen- trations of products to the equilibrium concentrations of reactants, each raised tothe power of its stoichiometric coefficient.

Equivalence point: The point at which the acid has completely reacted with or been neutralized by the base.

Indicators: Substances that have distinctly different colours in acidic and basic media.

Molar solubility: The number of moles of solute in one litre of a saturated solution (mol/L)

Monoprotic acid: Each unit of the acid yields one hydrogen ion upon ioniza- tion.

Neutralization reaction: A reaction between an acid and a base.

Precipitation reaction: A reaction that results in the formation of a precipitate.

Primary Standard: a high purity compound used to prepare the standard solution or to standardize the solution with.

Quantitative analysis: The determination of the amount of substances present in a sample.

Secondary Standard: a second material used as a substitute for a suitable primary standard. This standard solution should always be standardized using a primary standard.

Solubility product, Ksp: The equilibrium constant for the reaction in which a solid salt dissolves to give its constituent ions in solution. It expresses the equilibrium between a solid and its ions in solution.

Standardization: The process by which the concentration of a solution is determined.

Standard Solution: A solution of accurately known concentration.

Stoichiometry: The quantitative study of reactants and products in a chemical reaction.

Stoichiometric amounts: The exact molar amounts of reactants and products that appear in the balanced chemical equation.

Strong acids: Strong electrolytes which are assumed to ionize completely in water.

Strong bases: Strong electrolytes which are assumed to ionize completely in water.

Titration: The gradual addition of of a solution of accurately known concentration to another solution of unknown concentration until the chemical reaction between the two solutions is complete.

Volumetric methods of analysis: based on the measurement of the amount of reagent that combines with the analyte. The terms volumetric analysis specifically involves the determination of the volume of the reagent solution needed for a complete reaction.

Volumetric titrimetry: methods that require that a reagent solution of known concentration, standard solution or titrant, be used.

Acid-base indicators: acids or bases which exhibits a visual change on neutrali- zation by the basic or acidic titrant at or near the equivalence point.

Chelation: the process involved in formation of a chelate.

Chemical stoichiometry: measurement based on exact knowledge of chemical combination

Colorimetric indicator: intensely coloured substances in atleast one form (bound or unbound to a metal) and do change colour when the metal ion analyte binds with it.

Complex: a substance composed of two or more components capable of an independent existence.

Complexation: the association of two or more chemical species that are capable of independent existence by sharing one or more pairs of electrons.

Complexometric indicator: water soluble organic molecules that under go definite colour change in the presence of specific metal ions and are used incomplexometric titrations.

Complexometric titration: A titration based on the formation of coordination complexes between a metal ion and complexing agent (or chelating agent) to form soluble complexes.

Complexing agent or ligand: molecules and/or anions with one or more donor atoms that each donate a lone pair of electrons to the metal ion to form a covalent bond.

Coordination complex: a complex in which a central atom or ion is joined to one or more ligands through what is formally a coordinate covalent bond in which both of the bonding electrons are supplied by a ligand.

Metal chelate: a species that is simultaneously bound to two or more sites on a ligand.

Monodentate (or Unidentate) ligand: A ligand that shares a single pair of electrons with a central metal ion in a complex.

Multidentate ligand: A ligand which shares more than one pair of electrons with a central metal ion in a complex. Those ligands which share 2, 3, 4, 5, or 6 are referred to as bidentate, tridentate, tetradentate (or quadridentate), pentadentate (or quinqui dentate), and hexadentate, respectively.

Stability constant of a complex: a measure of the extent of formation of the complex at equilibrium.