8.1-8.4 Flashcards
acids
a substance that donates H+ to a solution
begins as a covalent (non-metal, non-metal) molecule
bases
a negative ion that can accept an H+ ion in solution or has at least one lone pair of electrons
a substance that donates OH- ions to a solution
amphoteric
can act as an acid and a base
ex. water
autoionization
the act of amphoteric substance’s molecules reacting with itself
reactants are favored
Kw
equilibrium expression for the autoionization of water
ion product constant for water
H3O+ is aka…
water with an H+ ion, or aqueous H+
if [H+] = [OH-]
the solution is neutral
if [H+] > [OH-]
the solution is acidic
if [H+] < [OH-]
the solution is basic
pH and pOH measure
how many ions per solution (concentration)
neutral pH
7
acidic pH
below 7 (0-7)
basic pH
above 7 (7-14)
[H+] = 10^
-pH
[OH-] = 10^
-pOH
Ka = 10^
-pKa
strong acids
pH close to zero
weak acids
pH close to 7
strong bases
pH close to 14
weak bases
pH close to 7
strong acids/bases
completely dissociate
dissociation is written…
with a single arrow (–>)
–the ions are NOT strong enough to react back and form the compound