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1120 buffer
1120 acid base
22 cards
Cards (90)
according to the
arrhenius
theory, an
acid
dissociates in water to give
H+
according to the
arrhenius
theory, a
base
dissociates in water to give
OH-
limitations of arrhenius theory
solvent can only be
water
cannot explain acid-base behaviour in
non aqueous
solution
cannot why all salts are
neutral
according to the
bronsted lowry
theory, an acid is a
proton donor
according to the
bronsted lowry
theory, a base is a
proton acceptor
a
bronsted
base must have
lone pair
electrons
according to the
lewis
theory, an acid is an
electron acceptor
according to the
lewis
theory, a base is an
electron donor
if water is
pure
and at
25
ºC ,
[
H3O+
] = [
OH−
] = 1 x 10^
-7
M
Kw
= [
H3O+
][
OH−
] = 1 x 10^
-14
M
pH =
-log
[
H+
]
pOH =
-log
[
OH−
]
at
25ºC
, pKw =
pH
+
pOH
=
14
Ka is the
acid ionisation constant
Kb is the
base ionisation constant
strong
acid/base has a
large
ionising
constant
(much
larger
than
1
)
weak
acid/base has a
small ionising constant
(much
smaller
than
1
)
Ka= [
H+
][
A-
]/[
HA
]
Kb= [
BH+
][
OH-
]/[
B
]
the
stronger
the acid, the
weaker
its conjugate base
the
stronger
the acid, the
larger
its Ka = the
smaller
its pKa
the
stronger
the base, the
larger
its Kb = the
smaller
its pKb
The percent
ionization
of a
weak
acid/base
increases
when the solution becomes more
dilute.
% ionisation = [
H+
] /
Initial
[
HA
] and then times 100%
percent ionization depends on:
Initial
molarity
ionization
constant
K <<<
1
=
backward
favoured
K >>>
1
=
forward
favoured
K = 1 =
equilibrium
Why does diluting the solution favour ionisation?
Concentration is given by
mole
/
volume.
If volume
increases
, it means that concentration will
decrease.
Concerning Ka = [H+][A-]/[HA] , the number of moles of ions in this equation must
increase
to maintain the constant
Ka.
(constant = unchanged)
Therefore this causes the equilibrium to shift to the
right
/
product
side, favouring
ionisation
contribution of self-ionization of water to pH can be ignored unless the solution is extremely
dilute
If the [
H+
] from the compound is
greater
than 1 x 10^-5 M, ignore
self
ionization
of
water
Polyprotic
acids are acids with more than one
ionizable
proton
(can donate multiple
H+
).
Each ionisation of
H+
of a polyprotic acid has its own
Ka
value
H3PO4
is a
triprotic
acid
Ka3
<
Ka2
<
Ka1
because it is more difficult to remove a
proton
from a more
negatively
charged species /
weaker
acid
Phosphoric Acid H3PO4 is a
weak
acid
Ka (
acid
) x Kb (its
conjugate base
) =
Kw
Kb
(base) x
Ka
(its
conjugate acid
) =
Kw
(constant)
In a conjugate acid base pair,
larger
Ka means a
smaller
Kb
In a conjugate acid base pair,
larger
Kb means a
smaller
Ka
When
salt
is dissolved in water, any pH change is caused by
hydrolysis
reaction
See all 90 cards
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