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Consider the weak bases below and their Kb values: C_6H_7O 48ptK_b=1.3 10^…
Related Topics
Wize University Chemistry Textbook > Acids and Bases
Base Equations (Kb, pKb)
1 Activity
Wize University Chemistry Textbook > Acids and Bases
Conjugate Acid-Base Pairs
2 Activities
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
C
5
H
5
N
K
b
=
1.7
×
10
−
9
C_5H_5N \hspace{40pt}K_b=1.7 \times 10^{-9}
C
5
H
5
N
K
b
=
1.7
×
1
0
−
9
Arrange the conjugate acids of these weak bases in order of increasing acid strength.
C
5
H
5
N
H
+
<
C
6
H
7
O
H
+
<
C
2
H
5
N
H
C_5H_5NH^+ < C_6H_7OH^+<C_2H_5NH
C
5
H
5
N
H
+
<
C
6
H
7
O
H
+
<
C
2
H
5
N
H
C
6
H
7
O
H
+
<
C
5
H
5
N
H
+
<
C
2
H
5
N
H
C_6H_7OH^+ < C_5H_5NH^+<C_2H_5NH
C
6
H
7
O
H
+
<
C
5
H
5
N
H
+
<
C
2
H
5
N
H
C
5
H
5
N
H
+
<
C
2
H
5
N
H
3
+
<
C
6
H
7
O
H
+
C_5H_5NH^+ < C_2H_5NH_3^+<C_6H_7OH^+
C
5
H
5
N
H
+
<
C
2
H
5
N
H
3
+
<
C
6
H
7
O
H
+
C
6
H
7
O
H
+
<
C
2
H
5
N
H
+
<
C
5
H
5
N
H
+
C_6H_7OH^+ < C_2H_5NH^+<C_5H_5NH^+
C
6
H
7
O
H
+
<
C
2
H
5
N
H
+
<
C
5
H
5
N
H
+
C
2
H
5
N
H
3
+
<
C
5
H
5
N
H
+
<
C
6
H
7
O
H
+
C_2H_5NH^+_3 < C_5H_5NH^+<C_6H_7OH^+
C
2
H
5
N
H
3
+
<
C
5
H
5
N
H
+
<
C
6
H
7
O
H
+
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More Base Equations (Kb, pKb) Questions:
Acids and Bases: Base equations
CH
3
NH
3
is a weak base. When mixed with water, we see the following reaction:
CH
3
NH
3
+ H
2
O <----> CH
3
NH
4
+
+ OH
-
Once the reaction reaches equilibrium, K
b
was found to be 1.07 x 10
-3
. If the reaction at equilibrium contains 2.5 M CH
3
NH
3
and 0.37 M CH
3
NH
4
+
, how much OH
-
is in solution?
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?
An aqueous solution only contains a 0.050 M in a weak base. Which of the following statements would be true about the solution?
Ammonia(NH
3
) is a weak base, K
b
= 1.8 x 10
-5
and benzoic acid (C
6
H
5
CH
2
O
-
) is a weak acid, K
a
= 6.3 x 10
-5
. A solution of ammonium benzoate (NH
4
)(C
6
H
5
CH
2
O
-
) is:
To 150 mL of water was added 0.18 moles of ammonia (NH
3
K
b
= 2.3 x 10
-5
) calculate the pH.
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,
Strength of Acids and Bases
What is the strongest acid below? What is the weakest acid?
Strongest acid:
Cl
3
CCOOH
Weakest acid:
HCN
Acids and Bases: Base Equations
Consider the weak bases below and their K
b
values:
C
6
H
7
O
K
b
=
1.3
×
10
−
10
C
2
H
5
N
H
2
K
b
=
5.6
×
10
−
4
C
5
H
5
N
K
b
=
1.7
×
10
−
9
\begin{alignedat}{} &C_6H_7O &&K_b = 1.3\times10^{-10}\\ &C_2H_5NH_2 &&K_b = 5.6\times10^{-4}\\ &C_5H_5N &&K_b = 1.7\times10^{-9} \end{alignedat}
C
6
H
7
O
C
2
H
5
N
H
2
C
5
H
5
N
K
b
=
1.3
×
1
0
−
10
K
b
=
5.6
×
1
0
−
4
K
b
=
1.7
×
1
0
−
9
Arrange the conjugate acids of these weak bases in order of
increasing
acid strength.
More Conjugate Acid-Base Pairs Questions:
In a reaction, which of the following could be conjugate acid-base pairs?
Weak Acids and Bases
Will HCO
3
-
act as an acid or as a base?
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**
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.