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General Chemistry MCAT
Acid/Base Equilibria
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Acid/ Base equilibria
General Chemistry MCAT > Acid/Base Equilibria
84 cards
Cards (110)
Bronsted-Lowry
Acid
Proton donor
(H+)
Bronsted-Lowry
Base
Proton
acceptor
Lewis Acid
Electron pair
Acceptor
Lewis Base
Electron pair donor
Buffer
An
aqueous
solution that resist changes in
pH
when added to an
acid
or
base
Buffers
Weak acid with
conjugate
base
Weak base with
conjugate
acid
Phosphate buffer
Commonly
used buffer
Ka
Acid
ionization constant/
acid
dissociation constant
Weak acid equilibrium
HF
(hydrofluoric acid): Ka=
3.5
x 10^
-4
CH3COOH
(acetic acid): Ka=
1.8
x 10^
-5
CH3OH
(methanol): Ka=
2.9
x 10^
-16
Weak base equilibrium
NH3
(Ammonia): Kb=
1.8
x 10^
-5
C6H5NH2
(Aniline): Kb=
4.3
x 10^
-10
Ka x Kb
Always equal Kw
Stronger
/
higher
Kb
The
weaker
Kb
pKa + pKb
=
14
Neutral salt solution
Neither the cation or anion will react in
water
or
solution
Neutral salt solutions
Ba(NO3)2
NaCl
Basic salt solution
The
cation
does not react in
water
, but the
anion
does
Basic salt solutions
Ba(CH3COO)2
NaClO
Acidic salt solution
The cation will react with
water
but the anion will not react with
water
Acidic salt solutions
NH4NO3
AlCl3
Acidic
,
Neutral
, or
Basic salt solution
The
cation
and
anion
both interact with
water
Acidic
,
Neutral
, or
Basic salt solution
(NH4)
2CO3
Increasing
the concentration of one of the products
Shifts the equilibrium to the
left
the
larger
the Ka value= the
stronger
the acid
the
smaller
the Ka value= the
weaker
the acid
the
larger
the Kb value= the
stronger
the base
the
smaller
the Kb value= the
weaker
the base
See all 110 cards