Study Set Content:
in pure water, the hydrogen and
hydroxyl ions concentration are
equal, and each has a value of
approximately
1 x 10-7 mole/liter
acids that donate a single proton
and bases that accept a single
proton
Monoprotic electrolyte
one that is capable of donating two
or more protons
Polyprotic(polybasis)acid
accepting two or more protons
Polyprotic(polyacidic) base
acid ionized in two stages:
Diprotic(dibasic)
Examples of Diprotic(dibasic)
Carbonic acid
○ Tartaric acid
ionizes in three stages:
Triprotic(Tribasic)
Triprotic(Tribasic)
Phosphoric acid
○ Citric acid
the hydrogen ion concentration of a
solution varies from approximately 1
in 1M solution of a strong acid to
about 1 x 10
-14
in a 1M solution of a
strong base, and the calculations
often become unwieldy.
Sorensen's pH
The neutral pH at 0 degrees celsius is
7.47
The neutral pH at 100 degrees celsius is
6.15
substance that liberates hydrogen
ions
Acid Arrhenius Theory
substance that supplies hydroxyl
ions on dissociation
Base Arrhenius Theory
happens because hydrogen ions
and hydroxide ions react to produce
water
Neutralization
H+(aq) + OH-(aq) →
H2O(I)
substance, charged or uncharged,
that is capable of accepting a proton
from acid
Base bronsted-Lowry theory
substance, charged or uncharged,
that is capable of donating a proton
to a base
Acid bronsted-Lowry theory
An acid must have a base present in order to function as an (blank), and vice versa
acid
a molecule or ion that accepts an
electron pair to form a covalent bond
Acid Lewis Theory
substance that provides the pair of
unshared electrons by which the
base coordinates with an acid, which
may be a proton (Bronsted-Lowrey),
or some other electron deficient
species
Base Lewis Theory
