Ionic Equilibrium Flashcards
What is ionic equilibrium?
A: Ionic equilibrium refers to the state in a solution where the concentrations of all ions remain constant over time due to the balance between the forward and reverse reactions.
Q: Define pH.
A: pH is the negative logarithm of the hydrogen ion concentration in a solution, given by
pH
=
β
log
β‘
[
π»
+
]
pH=βlog[H
+
].
Q: What is the relationship between pH and pOH?
A: pH and pOH are related by the equation
pH
+
pOH
=
14
pH+pOH=14 at 25Β°C (298 K).
What is the ionization constant of water (
πΎ
π€
K
w
β
)?
πΎ
π€
K
w
β
is the ionization constant of water, defined as
πΎ
π€
=
[
π»
+
]
[
π
π»
β
]
=
1
Γ
1
0
β
14
K
w
β
=[H
+
][OH
β
]=1Γ10
β14
at 25Β°C
Define a strong acid
A strong acid is one that completely dissociates in water, producing a high concentration of hydrogen ions (
π»
+
H
+
).
Give an example of a strong acid
Hydrochloric acid (HCl) is an example of a strong acid
Define a weak acid
A weak acid is one that partially dissociates in water, establishing an equilibrium between the undissociated acid and its ions.
Give an example of a weak acid
Acetic acid (CHβCOOH) is an example of a weak acid
What is the acid dissociation constant (
πΎ
π
K
a
β
)?
K
a
β
is a measure of the strength of an acid, defined as the equilibrium constant for the dissociation of an acid in water
How is pKa related to
πΎ
π
K
a
β
?
pKa=βlogK
a
β
. A lower pKa value indicates a stronger acid
Define a strong base.
A strong base is one that completely dissociates in water, producing a high concentration of hydroxide ions (
π
π»
β
OH
β
).
Give an example of a strong base.
Sodium hydroxide (NaOH) is an example of a strong base.
Define a weak base
A weak base is one that partially dissociates in water, establishing an equilibrium between the base and its ions.
Give an example of a weak base
Ammonia (NHβ) is an example of a weak base.
What is the base dissociation constant (
πΎ
π
K
b
β
)?
K
b
β
is a measure of the strength of a base, defined as the equilibrium constant for the dissociation of a base in water.
How is pKb related to
πΎ
π
K
b
β
?
pKb=βlogK
b
β
. A lower pKb value indicates a stronger base.
What is the common ion effect?
The common ion effect is the suppression of the ionization of a weak electrolyte when a strong electrolyte containing a common ion is added to the solution.
How does the common ion effect affect solubility?
The common ion effect decreases the solubility of a salt in solution by shifting the equilibrium towards the undissociated form
What is the buffer solution?
A buffer solution is one that resists changes in pH when small amounts of an acid or a base are added.
How is a buffer solution prepared?
A buffer solution is typically prepared by mixing a weak acid with its conjugate base or a weak base with its conjugate acid.
What is the Henderson-Hasselbalch equation for a buffer?
pH
pKa
+
log
β‘
(
[
A
β
]
[
HA
]
)
pH=pKa+log(
[HA]
[A
β
]
β
), where
[
A
β
]
[A
β
] is the concentration of the conjugate base and
[
HA
]
[HA] is the concentration of the acid.
Define solubility product (
πΎ
π
π
K
sp
β
).
K
sp
β
is the equilibrium constant for the dissolution of a sparingly soluble salt in water.
What is the relationship between solubility and
πΎ
π
π
K
sp
β
?
The solubility of a salt in water is directly related to the square root or cube root (depending on the stoichiometry) of its
πΎ
π
π
K
sp
β
.
What happens to the solubility of a salt if a common ion is added?
The solubility of a salt decreases if a common ion is added, due to the common ion effect.