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Molecular formula: Concentration
Related Topics
Wize University Chemistry Textbook > Acids and Bases
Autoionization of Water (Kw)
5 Activities
Wize University Chemistry Textbook > Acids and Bases
pH
4 Activities
A solution of HBr has a pOH of 12.2, what is the [H
+
] concentration?
2.4 x 10
-3
M
6.3 x 10
-13
M
12.2 M
1.6 x 10
-2
M
We can not find the [H
+
] from the pOH
I don't know
Check Submission
More Autoionization of Water (Kw) Questions:
Concentration
A solution of LiOH is made by mixing an unknown amount of LiOH with 1 L of water. The pOH is measured to be 3.65, what is the concentration of LiOH?
MW Li: 7 g/mol
MW O: 16 g/mol
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10
-10
) solution
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H
3
O
+
concentration in diet cola than in milk?
Acids and Bases: Ka
The following occurs when HCl is placed in water:
HCl <----> H
+
+ Cl
-
The K
a
for this reaction is known to be K
a
= 5.64 once it reaches equilibrium. At equilibrium, 1.35 x 10
-7
M of HCl and 1.2 M of Cl
-
can be found. What is the pH of the solution at equilibrium?
Acids and Bases: pH
100
m
L
100\ mL
100
m
L
of a
0.5
M
0.5\ M
0.5
M
solution of Hydrochloric acid (
H
C
l
\rm HCl
HCl
) was added to
48
m
L
48\ mL
48
m
L
of a
0.410
M
0.410\ M
0.410
M
solution of sodium benzoate (
C
6
H
5
C
O
O
N
a
\rm C_6H_5COONa
C
6
H
5
COONa
) the conjugate base of benzoic acid (
C
6
H
5
C
O
O
H
\rm C_6H_5COOH
C
6
H
5
COOH
K
a
=
6.6
×
10
−
5
\rm K_a = 6.6 \times 10^{-5}
K
a
=
6.6
×
1
0
−
5
). Calculate the
p
H
\rm pH
pH
of the resulting solution.
An aqueous solution only contains a 0.050 M in a weak base. Which of the following statements would be true about the solution?
Lactic acid, shown below, is added to many beverages, including some sour beers. What is the pH of a 0.050M lactic acid solution in 0.50M hydrochloric acid? (K
a
for lactic acid=1.38x10
-4
)
What is the hydroxide ion (OH
-
) concentration of a solution with a pH of 6.1?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K
a
= 4.9 x 10
-10
) solution
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H
3
O+ concentration in diet cola than in milk?
What is the pH of a solution prepared by mixing 50 mL of a 0.10 M HCl solution with 150 mL of pure water?
What is the pH of a 1.1M solution of nitrous acid (HNO
2
). The K
a
of nitrous acid is 7.2 x 10
-4
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H
3
O
+
concentration in diet cola than in milk?
Concentration
A solution of LiOH is made by mixing an unknown amount of LiOH with 1 L of water. The pOH is measured to be 3.65, what is the concentration of LiOH?
MW Li: 7 g/mol
MW O: 16 g/mol
pH: Neutralization
A student adds 11.6 mL of a 3.7M KOH solution, to 29 mL of a 1.4 M HCl. What is the final pH after the addition?
To 4.00 L of water was added 100 mg of HF (6.6 x 10
-4
). What is the pH?
CH
3
COOH is a weak acid with a K
a
of 1.8 x 10
-5
. In what pH range would you most likely an aqueous solution of Na(CH
3
COO).
To 150 mL of water was added 0.18 moles of ammonia (NH
3
K
b
= 2.3 x 10
-5
) calculate the pH.
Acids and Bases: Henderson Hasselbalch
To a solution of acetic acid (
K
a
=
1.8
×
10
−
5
\rm K_a = 1.8 \times 10^{-5}
K
a
=
1.8
×
1
0
−
5
) was added 0.1 mol of
N
a
O
H
\rm NaOH
NaOH
. After the addition of
N
a
O
H
\rm NaOH
NaOH
the volume was 1.4L and the
p
H
\rm pH
pH
was 5.2.
a) This solution a buffer? (True/False)
b) Calculate the number of moles of acetic acid that were originally in solution. Report your answer in moles to three significant figures. Do not include units in the answer field
What is the pH of a solution made by mixing 22g of NaOH in 3.1 L of water?
What is the pH of a solution of 0.1 M sodium acetate (NaCH
3
CO
2
) given that the Ka for acetic acid is 1.8×10
−5
?
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10
-10
) solution
To a
90
m
L
90\ mL
90
m
L
of
0.17
M
0.17\ M
0.17
M
of
H
F
\rm HF
HF
is added
25
m
L
25\ mL
25
m
L
of
0.06
M
0.06\ M
0.06
M
N
a
O
H
\rm NaOH
NaOH
. The
K
a
K_a
K
a
of
H
F
\rm HF
HF
is
7.2
×
10
−
4
7.2 \times 10^{-4}
7.2
×
1
0
−
4
. Calculate the
p
H
\rm pH
pH
of the solution.
What is the pH of pure, neutral water at 37°C? At 37°C, K
w
= 2.4x10
-14
.
A student titrated 10.00 mL of 0.10 M sodium acetate (CH
3
COONa) with HCℓ and determined that 10.00 mL of HCℓ was needed to reach the equivalence point. At equivalence, what is the expected pH?
K
a
of CH
3
COOH = 1.8×10
-5
Calculate the pH of the solution resulting from the addition of 10.0 mL of a 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 x 10
-10
) solution
What is the pH of a solution prepared by mixing 50 mL of a 0.10 M HCl solution with 150 mL of pure water?
The equilibrium constant for the auto-ionization of water at 10 °C is 3.0 x 10
-15
. What is the concentration of H
3
O
+
ions in pure water at this temperature?
If the pH of pure water is 6.80 at 37 °C, calculate K
w
pOH and [OH
-
] at this temperature.
Equilibrium: Auto-ionization of water
Given the equilibrium information for water below, what is the concentration of hydroxide ions in a solution of 1.5 M HCl?
2 H
2
O (l)
⇌
H
3
O+ (aq) + OH
-
(aq), K
c
= 1x10
-14
at 20
o
C
Equilibrium: ICE Tables and Auto-ionization of Water
Given the equilibrium information for water below, what is the concentration of hydroxide ions in water?
2 H
2
O (l) ⇌ H
3
O
+
(aq) + OH
-
(aq), K
c
= 1x10
-14
at 20
o
C
If the pH of pure water is 6.80 at 37 °C, calculate K
w
pOH and [OH
-
] at this temperature.
The compound
fluoroacetic acid
(shown), has a pK
a
value of 2.59. What is pK
b
of its conjugate base?
A solution of [CH
3
NH
3
][CH
3
COO] is made in an undergraduate laboratory. Use the information below to predict the acidity of the solution.
CH
3
COOH: K
a
= 1.8 x 10
-5
CH
3
NH
3
+
: K
a
= 2.3 x 10
-11
Auto-ionization of Water: pH
If the pH of pure water is 6.80 at 37 °C, calculate K
w
pOH and [OH
-
] at this temperature.
If an answer has an exponent (ex. 1.6x10
3
), input it as: 1.6e3
The equilibrium constant for the auto-ionization of water at 10 °C is 3.0 x 10
-15
. What is the concentration of H
3
O
+
ions in pure water at this temperature?
More pH Questions:
Weak Acids and Bases
Calculate the pH of the following solution.
A solution prepared by dissolving 4.25 x 10
-4
g of CH
3
COONa in 100.0 mL of water.
Note: Acetic Acid Ka = 1.8 x 10
-5
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a)
A 6.30 x 10
-2
M solution of CH
3
COOH in water.
b)
A solution prepared by dissolving 4.25 x 10
-4
g of CH
3
COONa in 100.0 mL of water.
Methyl diethanolamine CH
3
N(C
2
H
4
OH)
2
is a weak base which we will abbreviate as
mdea
. The conjugate acid,
mdeaH
+
, has a pKa = 8.52.
Henderson Hasselbalch: Titrations and pH
For the titration of 50.00 mL of 0.1000 M ammonia (NH
3
) with 0.1000 M HCl calculate the pH
(
F
o
r
a
m
m
o
n
i
a
K
b
=
1.8
×
10
−
5
)
(For\ ammonia\ Kb=1.8\times10^{-5})
(
F
or
amm
o
nia
K
b
=
1.8
×
1
0
−
5
)
Before the addition of any HCl
After 20.00 mL of the acid has been added
100 mL of a 0.5 M solution of nitric acid (
H
N
O
3
\rm HNO_3
HN
O
3
) was added to 75 mL of a 0.37 M solution of sodium benzoate (
C
6
H
5
C
O
O
N
a
\rm C_6H_5COONa
C
6
H
5
COONa
) the conjugate base of benzoic acid (
C
6
H
5
C
O
O
H
K
a
=
6.6
×
10
−
5
\rm C_6H_5COOH Ka = 6.6 \times 10^{-5}
C
6
H
5
COOHKa
=
6.6
×
1
0
−
5
). Calculate the
p
H
\rm pH
pH
of the resulting solution.
If the pH of pure water is 6.80 at 37 °C, calculate K
w
pOH and [OH
-
] at this temperature.
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H
3
O
+
], pH and pOH of the solution
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H
3
O
+
], pH and pOH of the solution
Acids and Bases: pH of Alkaline Earth Metal Hydroxides
Calculate the pH of a 1.00 x 10
-4
M Mg(OH)
2
solution.
Acids and Bases: Strong Acid Mixture
Practice Question: Strong Base Mixture
Calculate the pH and pOH of a solution containing a mixture of 75.00 mL of 0.100 M HI and 25.00 mL of 0.250 M HClO
4
.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.500 g of sodium hydrogen phosphate (Na
2
HPO
4
, MW = 141.9579 g/mol) in 150.0 mL of water.
Weak Acids and Bases
Calculate the pH and pOH of the following solutions.
a)
A 6.30 x 10
-2
M solution of CH
3
COOH in water.
b)
A solution prepared by dissolving 4.25 x 10
-4
g of CH
3
COONa in 100.0 mL of water.
Strong Acids and Bases
Calculate the pH of a basic solution prepared by taking 10.00 mL of 0.700 M NaOH solution and diluting it to 100.00 mL with water.
Strong Acids and Bases
Calculate the pH of a solution prepared by adding 100.0 mL of 3.00 x 10
-2
M KOH with 50.0 mL of 2.50 x 10
-2
M Be(OH)
2
.
Strong Acids and Bases
Calculate the pH and pOH of the following solutions.
a)
2.75 x 10
-3
M aqueous HNO
3
solution.
b)
1.50 x 10
-2
g of CaO dissolved in 200.0 mL of water.
Weak Acids and Bases
Calculate the pH and pOH of the following solutions, knowing that Ka = 1.8x10^-5.
a)
A 5.33 x 10
-2
M solution of CH
3
COOH in water.
b)
A solution prepared by dissolving 1.15 x 10
-3
g of CH
3
COONa in 100.0 mL of water.
Weak Acids and Bases
Calculate the pH of a solution prepared by dissolving 0.150 g of sodium hydrogen phosphate (Na
2
HPO
4
, MW = 141.9579 g/mol) in 125.0 mL of water.
K
a
(
H
P
O
4
2
−
)
=
4.2
x
10
−
13
;
K
b
(
H
P
O
4
2
−
)
=
1.6
x
10
−
7
.
K_a\ \left(HPO_4^{2-}\right)\ =\ 4.2\ x\ 10^{-13};\ \ K_b\ \left(HPO_4^{2-}\right)\ =\ 1.6\ x\ 10^{-7}.\
K
a
(
H
P
O
4
2
−
)
=
4.2
x
1
0
−
13
;
K
b
(
H
P
O
4
2
−
)
=
1.6
x
1
0
−
7
.
Strong Acids and Bases
Calculate the pH of a basic solution prepared by taking 20.00 mL of 0.500 M Be(OH)
2
solution and diluting it to 100.00 mL with water.
Strong Acids and Bases
Calculate the pH of a solution prepared by adding 25.00 mL of 0.100 M HCl with 75.00 mL of 2.50 x 10
-2
M HBr.
Strong Acids and Bases
Calculate the pH and pOH of the following solutions.
a)
3.00 x 10
-4
M aqueous HClO
4
solution.
b)
8.00 x 10
-3
g of Na
2
O dissolved in 150.0 mL of water.
Consider the following reaction in water:
NaOH <----> Na
+
+ OH
-
This reaction has a Kb of 1 x 10
-10
and a pOH of 3. If there is 1 M of NaOH at equilibrium, what is the concentration of Na
+
in solution?
Acids and Bases: pH based on % dissociation
In a 0.25 M solution, a weak acid is 3.0% dissociated. Calculate [H
3
O
+
], pH and pOH of the solution
If an answer is an exponent such as 4.3x10
-7
, input the answer as: 4.3e-7
Which of the solutions below would have the HIGHEST pH value?
Acids and Bases: pH
What is the pH of a 0.10 M solution of NaF? (K
a
for HF = 6.8×10
-4
)?
Methyl diethanolamine CH
3
N(C
2
H
4
OH)
2
is a weak base which we will abbreviate as
mdea
. The conjugate acid,
mdeaH
+
, has a pKa = 8.52.