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Weak Acids and Bases
Related Topics
Wize University Chemistry Textbook > Acids and Bases
Applications of Acid and Base Equations
3 Activities
Wize University Chemistry Textbook > Acids and Bases
Conjugate Acid-Base Pairs
2 Activities
Will HCO
3
-
act as an acid or as a base?
Answer
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
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
)
Acids and Bases: pH
What is the pH of a 0.10 M solution of NaF? (K
a
for HF = 6.8×10
-4
)?
More Conjugate Acid-Base Pairs Questions:
In a reaction, which of the following could be conjugate acid-base pairs?
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?
In the reaction
H
S
O
4
−
(
a
q
)
+
O
H
−
(
a
q
)
⇌
S
O
4
2
−
(
a
q
)
+
H
2
O
(
l
)
HSO_4^-\left(aq\right)\ +\ OH^-\left(aq\right)\ ⇌\ SO_4^{2-}\left(aq\right)\ +\ H_2O\ \left(l\right)
H
S
O
4
−
(
a
q
)
+
O
H
−
(
a
q
)
⇌
S
O
4
2
−
(
a
q
)
+
H
2
O
(
l
)
the conjugate acid-base pairs are
Select which of the following WOULD NOT be a conjugate acid/base pair.
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
Consider the following reaction:
N
H
4
+
+
O
H
−
⇌
H
2
O
+
N
H
3
NH^{4+}+OH^-\rightleftharpoons H_2O+NH_3
N
H
4
+
+
O
H
−
⇌
H
2
O
+
N
H
3
Choose the INCORRECT statement
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
H
C
l
+
H
2
O
⇌
\rm HCl\quad+\quad H_2O\quad \xrightleftharpoons{\hspace{1.5cm}}
HCl
+
H
2
O
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
Consider the weak bases below and their K
b
values:
C
6
H
7
O
K
b
=
1.3
×
10
−
10
C_6H_7O \hspace{48pt}K_b=1.3 \times 10^{-10}
C
6
H
7
O
K
b
=
1.3
×
1
0
−
10
C
2
H
5
N
H
2
K
b
=
5.6
×
10
−
4
C_2H_5NH_2 \hspace{30pt}K_b=5.6 \times 10^{-4}
C
2
H
5
N
H
2
K
b
=
5.6
×
1
0
−
4
In the reaction
H
S
O
4
(
a
q
)
−
+
O
H
(
a
q
)
−
⇌
S
O
4
(
a
q
)
2
−
+
H
2
O
(
l
)
HSO^-_{4(aq)}+OH^-_{(aq)} \rightleftharpoons SO^{2-}_{4(aq)}+H_2O_{(l)}
H
S
O
4
(
a
q
)
−
+
O
H
(
a
q
)
−
⇌
S
O
4
(
a
q
)
2
−
+
H
2
O
(
l
)
the conjugate acid-base pairs are
To 2L of pure water is added Mg(ClO
4
)
2
. What would the effect on pH be?
Triemethylamine (N(CH
3
)
3
) is a base (pKb=4.19) used in a variety of organic reactions. It can also be used as an effective Lewis base due to it's small steric profile.
if a solution of [N(CH
3
)
3
H]
2
[SO
4
]is dissolved in neutral water the pH will be,
A series of solutions are formed with strontium salts of the form SrX
2
where X=F, Cl, Br, I.
Which of the solutions will have the highest pH?
Pure water has a pH of 7.00. 1.1g of MgBr
2
is added to 15L of pure water. The solubility of MgBr
2
in water is approximatly 101.5g/L. What is the pH of the resulting solution?
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
H
C
l
+
N
H
3
⇌
\rm HCl\quad+\quad {NH_3}\quad \xrightleftharpoons{\hspace{1.5cm}}
HCl
+
N
H
3
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
+
C
H
3
C
O
O
H
⇌
H
2
O
+
N
a
+
C
H
3
C
O
O
−
\rm \quad+\quad {CH_3COOH}\quad \xrightleftharpoons{\hspace{1.5cm}}\quad H_2O\quad+\quad Na^+CH_3COO^-
+
C
H
3
COOH
H
2
O
+
N
a
+
C
H
3
CO
O
−
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
Acids and Bases: Conjugate
In each equation, label the acids, bases and conjugate acid-base pairs
N
H
3
+
H
3
P
O
4
↔
N
H
4
+
+
H
2
P
O
4
−
NH_3+H_3PO_4 \leftrightarrow NH^+_4+H_2PO^-_4
N
H
3
+
H
3
P
O
4
↔
N
H
4
+
+
H
2
P
O
4
−
C
H
3
O
−
+
N
H
3
↔
C
H
3
O
H
+
N
H
2
−
CH_3O^-+NH_3 \leftrightarrow CH_3OH+NH^-_2
C
H
3
O
−
+
N
H
3
↔
C
H
3
O
H
+
N
H
2
−
Using the incomplete reaction below, choose the completed equilibrium which indicates the correct association of conjugate acid base pairs.
H
C
l
+
H
2
O
⇌
\rm HCl\quad+\quad H_2O\quad \xrightleftharpoons{\hspace{1.5cm}}
HCl
+
H
2
O
**#1 and #2 designate the two sets of conjugate acid base pairs present in each equilibrium**
Acids and Bases: Conjugate
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 \rm 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}
Acid
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
Acids and bases: Conjugate identification
In the reaction HSO
4
-
(aq) + OH
-
(aq) ⇌ SO
4
2
-(aq) + H
2
0(l), the conjugate acid-base pairs are:
B is a weak base. Which equilibrium corresponds to the equilibrium constant K
a
for HB
+
?
Acids and Bases: Conjugate Acid-base Pairs
Indicate how many of these combinations are conjugate acid-base pairs.
Select all that apply.