General Chemistry - Acids and bases

Chapter 10 MCAT (terms)

Arrhenius acid

will dissociate to form an excess H+ in solution

Arrhenius base

will dissociate to form an excess OH- in solution

Bronsted Lowry Acid

species donates hydrogen ions

Bronsted Lowry base

species accepts hydrogen ions

Lewis Acid

electron pair receptor

Lewis Base

Electron pair donor

Amphoteric species

reacts like an acid in basic environment and basic in acidic environemtn

pH

concentration of hydrogen ions

pOH

concentration of hydroxide ions

strong acids/bases

completely dissociate into their component ions in aqueous solution

Conjugate acid

acid formed when a base gains a proton

Conjugate base

is the base fortmed when acid loses a proton

acid equvalent

one mole of H+ ions

base equivalent

one mole of OH- ions

Polyvalent

each mole of the acid or base is more than one acid or base equivalent

Titration

procedure used to determine the concentration of a known reactant in a solution

equivalence point

number of acid equivalent presents in the original solution equals the number of base equivalents added

Strong acid and weak base equivalent point

pH < 7

Strong acid and strong base equivalence point

pH = 7

Weak acid and strong base equivalence point

pH > 7

Half equivalence point

the midpoint of the buffering region, in which half of the titrant has been protanated

Region I

little acid added, predominant species is CO32-

Region II

More acid added, predominant species are CO23- or HCO3- in relatively equal concentrations

Region III

equivalence point, all CO23- titrated to HCO3-

Region IV

Acid neutrated half of HCO3- and now H2CO3 and HCO3- are roughly equal cocnentrations

Region V

Second equivalence point all HCO3- is now H2CO3

Bicarbonate buffer solution

H2CO3/HCO3- plasma compoent of blood

Buffering capcity

ability to which system can resist changers in pH