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The ion product of water,
K
w is the equilibrium constant for the autoionization reaction:
Key equations
-
K
w = [H
3 O
+ ][OH
− ] = 1.0
10
−14 (at 25 °C)
Chemistry end of chapter exercises
Write equations that show NH
3 as both a conjugate acid and a conjugate base.
One example for NH
3 as a conjugate acid:
as a conjugate base:
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Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry acid:
(a)
(b) HCl
(c) NH
3
(d) CH
3 CO
2 H
(e)
(f)
(a)
(b)
(c)
(d)
(e)
(f)
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Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry acid:
(a) HNO
3
(b)
(c) H
2 S
(d) CH
3 CH
2 COOH
(e)
(f) HS
−
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Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry base:
(a) H
2 O
(b) OH
−
(c) NH
3
(d) CN
−
(e) S
2−
(f)
(a)
(b)
(c)
(d)
(e)
(f)
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Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry base:
(a) HS
−
(b)
(c)
(d) C
2 H
5 OH
(e) O
2−
(f)
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What is the conjugate acid of each of the following? What is the conjugate base of each?
(a) OH
−
(b) H
2 O
(c)
(d) NH
3
(e)
(f) H
2 O
2
(g) HS
−
(h)
(a) H
2 O, O
2− ; (b) H
3 O
+ , OH
− ; (c) H
2 CO
3 ,
(d)
(e) H
2 SO
4 ,
(f)
(g) H
2 S; S
2− ; (h)
H
4 N
2
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What is the conjugate acid of each of the following? What is the conjugate base of each?
(a) H
2 S
(b)
(c) PH
3
(d) HS
−
(e)
(f)
(g) H
4 N
2
(h) CH
3 OH
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Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:
(a)
(b)
(c)
(d)
(e)
(f)
(g)
The labels are Brønsted-Lowry acid = BA; its conjugate base = CB; Brønsted-Lowry base = BB; its conjugate acid = CA. (a) HNO
3 (BA), H
2 O(BB), H
3 O
+ (CA),
(b) CN
− (BB), H
2 O(BA), HCN(CA), OH
− (CB); (c) H
2 SO
4 (BA), Cl
− (BB), HCl(CA),
(d)
OH
− (BB),
(CB), H
2 O(CA); (e) O
2− (BB), H
2 O(BA) OH
− (CB and CA); (f) [Cu(H
2 O)
3 (OH)]
+ (BB), [Al(H
2 O)
6 ]
3+ (BA), [Cu(H
2 O)
4 ]
2+ (CA), [Al(H
2 O)
5 (OH)]
2+ (CB); (g) H
2 S(BA),
HS
− (CB), NH
3 (CA)
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Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:
(a)
(b)
(c)
(d)
(e)
(f)
(g)
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What are amphiprotic species? Illustrate with suitable equations.
Amphiprotic species may either gain or lose a proton in a chemical reaction, thus acting as a base or an acid. An example is H
2 O. As an acid:
As a base:
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State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species:
(a) H
2 O
(b)
(c) S
2−
(d)
(e)
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State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species.
(a) NH
3
(b)
(c) Br
−
(d)
(e)
amphiprotic: (a)
(b)
not amphiprotic: (c) Br
− ; (d)
(e)
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Source:
OpenStax, Chemistry. OpenStax CNX. May 20, 2015 Download for free at http://legacy.cnx.org/content/col11760/1.9
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