Section 20.10 Acid-Base Buffers
Name:
Date:
A. I
1. A basic buffer solution can be prepared by mixing equal
numbers of moles of 9601
A. NH4Cl and HCl
B. NaCl and NaOH
C. Na2CO3 and NaHCO3
D. NaCH3COO and
CH3COOH
2. A few drops of strong acid are added to 1.0 L of a pH 8.0
buffer solution. The resulting solution will have an approximate
pH of 9604
A. 5.6
B. 7.0
C. 7.9
D. 8.1
B. II
C. III
D. IV
9. Consider the following: 9708

A buffer solution is prepared by adding NaCH 3 COO s to
CH3COOH(aq). When a few drops of NaOH solution are
added to the buffer, the equilibrium
3. Which of the following would produce a buffer solution when
added to 1.0 M NH3 ? 9604
A. HNO3
B. KNH2
C. NaOH
D. NH4Cl
4. Which of the following pairs of substances form a buffer
system for human blood? 9608
A. HCl and Cl 
B. NH3 and NH2

C. H2CO3 and HCO3
D. H3C6H5O7 and HC6H5O7

5. A buffer solution is prepared by adding 1.0 mol of
NaCH3COO to 1.0 L of 1.0 M CH3COOH. The molar
[CH3COOis approximately 9701
CH3COOH + H2O qwe CH3COO– + H3O+
1.0M
1.0M
A. 0.0
B. 0.5
C. 1.0
10. Which of the following could be used to form a buffer
solution? 9801
A. HBr and NaOH
B. HCl and NH4Cl
C. HNO3 and NaNO3
D. H2CO3 and NaHCO3

11. A buffer solution can be prepared by combining, in water,
equal moles of 9804
A. HF and KF
B. HIO3 and HI
C. HBr and LiBr
D. HClO4 and NaOH
12. Consider the following equilibrium for a buffer solution:
9806
D. 2.0
6. A buffer solution can be prepared from 9704
A. nitric acid and sodium nitrate.
B. sulphuric acid and sodium hydroxide.
C. hydrocyanic acid and sodium cyanide.
D. sodium hydroxide and sodium chloride.

When a small amount of acid is added to this system, and
equilibrium is reestablished,
7. Consider the following equilibrium for a buffer solution: 9704
When a few drops of HCl are added,
8. Consider the following titration curve for the neutralization of
CH3COOH by KOH: 9706
13. A buffer solution can be prepared by combining equal
moles of a 9808
A. strong acid and a strong base.
B. weak acid and its conjugate base.
C. strong base and its conjugate acid.
D. strong acid and its conjugate base.
14. A buffer solution can be formed by dissolving equal moles
of 9901
A. HF and NaF
B. HCl and NaOH
C. KBr and Na3PO4
D. CH3COOH and NaCl
15. Calculate the [H3Oin a solution prepared by mixing
25.0 mL of 1.0 M HCl with 50.0 mL of 0.50 M KOH.
0.025moles HCl
A. 1. 0 M
On the graph above, the solution is buffered at point
Section -Document1 p 1 o f 3
0.025mole KOH
B. 0.50 M
C. 0.25 M
D. 1.010–7 M
16. A buffer solution is formed by adding which of the
following to water? 9904
A. HCl and KOH
B. HCN and RbCN
C. NaBr and NaOH
D. HNO3 and LiNO3
17. Consider the following: 9906
I. H3O
II. CH3COO
III. CH3COOH
The purpose of a buffer system consisting of CH3COOH and
CH3COONa is to maintain a relatively constant [ ] of
A. I only.
B. I and II only.
C. II and III only.
D. I, II and III.
18. Consider the following graph for the titration of 9908
1.C 2.C
3.D 4.C 5.C 6.C 7.C
8.B 9.C 10.D 11.A
12.C 13.B 14.A 15.D
16.B 17.A 18.B 19.D
20.B
20-10 MC ANS:
PART B: Written Response:
A buffer solution is present at point
A. I
B. II
C. III
D. IV
19. Which of the following graphs describes the relationship
between the pH of a buffer and the volume of NaOH added to
the buffer? 0001
1. A 2.0 L solution contains one mole of the weak acid,
H3PO4, in equilibrium with one mole of the salt, NaH2PO4,
a) Write an equation that represents this equilibrium. (2
marks) 9606
A: H3PO4 + H2O qe H2PO4- + H3O+
b) Explain why the pH of this solution does not change
significantly when 10.0 mL of 1.0 M KOH is added. (1 mark)
The moles of OH– is small compared to
the moles of weak acid in the buffer, so
the buffer reacts with it and holds pH
constant.
20. Which of the following graphs describes the relationship
between pH of a buffer solution and a volume of HCl added to
the buffer? 0006
Section -Document1 p 2 o f 3
There is 1.0 mol H3PO4 and 1.0 mol
H2PO4
The 10.0mL 1.0M KOH is 0.01mol OH–
H3PO4 + H2O qe H2PO4- + H3O+
1.0mol
1.0 mol
-0.01 mol
+0.01mol
0.99
1.01
Section 20.11 Acid-Base Applications
Name:
1. The pH range of ‘acid rain’ is often 9601
A. 3 to 6
B. 6 to 8
C. 7 to 9
Date:
D. 10 to 12
2. Sulphur dioxide gas forms an acidic solution. The equation
representing this reaction is
3. Which of the following is primarily responsible for acid rain?
9606
A. HCl
B. H2SO4
C. HClO4
D. CH3COOH
4. Normal rainwater has a pH of approximately 6 as a result of
dissolved 9704 9801 9901
A. oxygen.
B. carbon dioxide.
C. sulphur dioxide.
D. nitrogen dioxide.
E. ammonia
5. Which of the following could be the pH of a sample of acid
rain? 9808
A. 0
B. 4
C. 7
D. 10
6. Which of the following gases is a contributor to the formation
of acid rain? 9901
A. H2
B. O3
C. SO2
D. NH3
7. A gas which is produced by internal combustion engines and
contributes to the formation of acid rain is 0001
A. H2
B. O3
C. CH4
D. NO2
MC ANS: 1.A 2.A 3.B 4.B
5.B 6.C 7.D
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