Exam Three Vocabulary Flashcards
properties of acids
dissolve metals, sour taste
properties of bases
slippery feel, bitter taste
Arrhenius Theory
acid: substance that increases H+ in water
base: substance that increases OH- in water
Bronstead-Lowry Theory
acid: proton donor
base: proton acceptor
always occur together
Conjugate Acid
has one more proton than the base from which it forms
Conjugate Base
has one less proton than the acid from which it forms
6 strong acids
HClO4
HCl
HBr
HI
HNO3
H2SO4
6 strong bases
LiOH
NaOH
KOH
Ca(OH)2
Sr(OH)2
Ba(OH)2
weak acids
donate some available protons
establish an equilibrium with the conjugate
the weaker the acid or base…
the stronger its conjugate
amphoteric
can be acid OR base
amphiprotic
can accept OR donate protons
basic solution
low pH
acidic solution
high pH
pH + pOH = pKw
Ka
acid dissociation constant
pH = -log[H+]
polyprotic acids
multiple donate able protons per acid molecule
diuretic acid
2 donatable protons per acid molecule
triprotic acid
3 donatable protons per acid molecule
weak bases
accepts some of the available protons
types of weak bases
conjugate bases of weak acids
ammonia and amines
Lewis Acid-Base Theory
lewis acid: accepts an electron pair
lewis base: donates an electron pair
coordinate covalent bond
both of the shared (B.P. e-) originate with the same atom
buffer
mixture of appreciable amounts of a weak acid-base pair the pH of a buffer resists change when small amounts of acid or base are added
Henderson-Hasselbach equation
pH = pKa + log [A-]/[HA]
effect of acid/base addition
neutralization
dilution
equilibrium
