acid and bases vocab

binary acid

acid that contains hydrogen and a more electronegative nonmetal

ternary acid

acid containing hydrogen and a polyatomic ion

arrhenius acid

a compound that dissociates in water to produce hydronium or hydrogen ions

arrhenius base

a compound that dissolves in water to produce hydroxide

strong acid

an acid that dissociates completely in an aqueous solution

weak acid

an acid that dissociates partially in water (equilibrium)

strong electrolyte

bases that dissociate completely in aqueous solutions

weak electrolyte

bases that ionizes partially in an aqueous solution (equilibrium)

bronsted-lowry acid

molecule or ion that is a proton donor

bronsted-lowry base

molecule or ion that is a proton acceptor

monoprotic acid

acid containing 1 hydrogen atom

polyprotic acid

molecule containing more than one hydrogen atom

diprotic acid

molecule containing 2 hydrogen atoms

triprotic acid

molecule containing 3 hydrogen atoms

lewis acid

a compound that accepts electrons

lewis base

a molecule that donates electrons

conjugate base

the ion or molecule that remains after an acid loses a proton / H+

conjugate acid

the ion or molecule formed when a base gains a proton / H+

amphoteric compound

a compound where water can act as an acid or a base depending on the strength of the acid or base with which it is reacting with (ex. H2O)

salt

ionic compound composed of a cation from a base and an anion from an acid

self-ionization of water

one water molecule transfers a H+ ion to a second water molecule, forming a H3O+ ion and an OH- ion

pH

a measure of the hydrogen ion concentration of a solution

pOH

a measure of the hydroxide ion concentration of a solution

Ka

the equilibrium constant for the ionization of a weak acid, measures strength of the acid

Kb

the equilibrium constant for the ionization of a weak base, measures strength of a base

titration

a method used to determine the concentration of a solution by reacting a known volume of the solution with absolute solution of known concentration

equivalence point

the point at which moles of H+ ion from the acid equal moles of OH- ion from the base

endpoint

the point where the pH indicator changes color when trying to find the equivalence point

standard solution

where a clean buret is filled with the titrating solution of known concentration