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Acids and Bases: pH
Related Topics
Wize University Chemistry Textbook > Acids and Bases
Applications of Acid and Base Equations
3 Activities
Wize University Chemistry Textbook > Acids and Bases
pH
4 Activities
What is the pH of a 0.10 M solution of NaF? (K
a
for HF = 6.8×10
-4
)?
2.08
5.92
8.08
11.92
I don't know
Check Submission
More Applications of Acid and Base Equations 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.
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.
Weak Acids and Bases
Will HCO
3
-
act as an acid or as a base?
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
.
Weak Acids and Bases
Calculate the percent dissociation for the following solutions.
a)
A 0.444 M aqueous solution of HCN (
K
a
= 6.2 x 10
-10
).
b)
A 3.50 x 10
-2
M aqueous solution of NaCN.
Weak Acids and Bases
Sulfurous acid (H2SO
3
) is a diprotic weak acid (p
K
a1
= 1.85, p
K
a2
= 7.20). Bisulfite (HSO
3
-
) is the conjugate base of sulfurous acid and is an amphoteric species (can act as an acid or a base). Will HSO
3
-
act as an acid or as a base?
Using the data in the table, which of the conjugate bases below is the strongest base?
A
c
i
d
K
a
H
O
A
c
1.8
×
10
−
5
H
C
H
O
2
1.8
×
10
−
4
H
C
l
O
3.0
×
10
−
8
H
F
6.8
×
10
−
4
\def\arraystretch{1.5} \begin{array}{c} \hline Acid &&&K_a\\ \hline HOAc&&&1.8 \times 10^{-5}\\ HCHO_2&&&1.8 \times 10^{-4}\\ HClO &&& 3.0 \times 10^{-8}\\ HF &&& 6.8 \times 10^{-4}\\ \hline \end{array}
A
c
i
d
H
O
A
c
H
C
H
O
2
H
C
l
O
H
F
K
a
1.8
×
1
0
−
5
1.8
×
1
0
−
4
3.0
×
1
0
−
8
6.8
×
1
0
−
4
Consider the weak bases below and their K
b
values:
C
6
H
7
O K
b
= 1.3 x 10
-10
C
2
H
5
NH
2
K
b
= 5.6 x 10
-4
Acids and Bases
Find the pH during titration of 20.00 mL of 0.100 M butanoic acid with 0.100 M NaOH solution after the following additions of base: 0 mL, 10.00 mL, 20.00 mL, 25.00 mL (K
a
= 1.54 x 10
-5
)
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
Molecular formula: Concentration
A solution of HBr has a pOH of 12.2, what is the [H
+
] concentration?
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?
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.