unit four: stoichiometry

stoichiometry

the process of using a balanced chemical equation to calculate the relative masses of reactants and products involved in a reaction; founded on the law of conservation of mass

solution

a homogenous mixture of two or more pure substances

aqueous solution

a solution in which water is the solvent

electrolyte

a substance that forms ions (charged particles) when dissolved in water — have ions!

strong electrolyte

an electrolyte that dissociates completely when dissolving in water (more ions)
ionic compounds — metal/nonmetal, metal/polyatomic, polyatomic/nonmetal, polyatomic/polyatomic, strong acids

weak electrolyte

an electrolyte that dissociates partially when dissolving in water (fewer ions)

non-electrolyte

a substance that does not form ions when dissolved in water (basically doesn't dissolve in water; eg. sugar) — do not have ions! — molecular compounds

solvation

the process of surrounding solute particles with solvent particles to form a solution

precipitation reaction

a reaction in which an insoluble substance forms and separates from the solution

ionic compound

a compound that dissolves by dissociation where water molecules surround the separated ions

molecular compound

a compound that interacts with water molecules but most do not dissociate

spectator ion

an ion that appears on both sides of an equation but is not directly involved in the reaction

base

proton acceptor

acid

proton donor

acid-base reaction/neutralization reaction

a reaction in which an acid reacts with a base and the two neutralize each other, producing water

oxidation-reduction reaction/redox reaction

reaction — OIL RIG
loss of electrons: oxidation
gain of electrons: reduction

solubility

the ability of one substance to dissolve in another

strong base

a base that dissociates completely into ions in solution

weak base

a base that does not dissociate completely into ions in solution

titration

a measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete

standard solution

a solution whose concentration is known

salt

an ionic compound made from the neutralization of an acid with a base

concentration

a measurement of how much solute exists within a certain volume of solvent

molarity

the number of moles of solute per liter of solution

dilution

adding water to a solution in order to decrease the concentration

equivalence point

the point at which the two solutions used in a titration are present in chemically equivalent amounts