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2006 Chapter 16 Acid-Base Titration and pH Study Guide


Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

1. 
Pure water contains
a.
water molecules only.
b.
hydronium ions only.
c.
hydroxide ions only.
d.
water molecules, hydronium ions, and hydroxide ions.
 

2. 
Pure water partially breaks down into charged particles in a process called
a.
hydration.
c.
self-ionization.
b.
hydrolysis.
d.
dissociation.
 

3. 
What is the concentration of H3O+ in pure water?
a.
10–7 M
c.
55.4 M
b.
0.7 M
d.
107 M
 

4. 
What is the product of H3O+ and OH– concentrations in water?
a.
10–28
c.
10–7
b.
10–14
d.
55.4
 

5. 
Which expression represents the concentration of H3O+ in solution?
a.
10–14 – [OH–]
c.
10–14 ¸ [OH–]
b.
10–14 ´ [OH–]
d.
[OH–] ¸ 10–14
 

6. 
Which expression represents the concentration of OH– in solution?
a.
10–14 – [H3O+]
c.
10–14 ¸ [H3O+]
b.
10–14 ´ [H3O+]
d.
[OH–] ¸ 10–14
 

7. 
If [H3O+] of a solution is greater than [OH–], the solution
a.
is always acidic.
c.
is always neutral.
b.
is always basic.
d.
might be acidic, basic, or neutral.
 

8. 
If [H3O+] of a solution is less than [OH–], the solution
a.
is always acidic.
c.
is always neutral.
b.
is always basic.
d.
might be acidic, basic, or neutral.
 

9. 
The common logarithm of a number, N, is the
a.
inverse of N.
b.
square root of N.
c.
power to which N must be raised to equal 10.
d.
power to which 10 must be raised to equal N.
 

10. 
The antilogarithm of a number, y, is
a.
the inverse of y.
c.
y raised to the power of 10.
b.
the square root of y.
d.
10 raised to the power of y.
 

11. 
What is the pH of a neutral solution at 25ºC?
a.
0
c.
7
b.
1
d.
14
 

12. 
The pH scale in general use ranges from
a.
0 to 1.
c.
0 to 7.
b.
–1 to 1.
d.
0 to 14.
 

13. 
The pH of an acidic solution is
a.
less than 0.
c.
greater than 7.
b.
less than 7.
d.
greater than 14.
 

14. 
The pH of a basic solution is
a.
less than 0.
c.
greater than 7.
b.
less than 7.
d.
greater than 14.
 

15. 
A water solution whose pH is 10
a.
is always neutral.
c.
is always acidic.
b.
is always basic.
d.
might be neutral, basic, or acidic.
 

16. 
A water solution whose pH is 7
a.
is always neutral.
c.
is always acidic.
b.
is always basic.
d.
might be neutral, basic, or acidic.
 

17. 
To calculate the pH of a solution whose [OH–] is known, first calculate
a.
[H3O+].
c.
antilog[H3O+].
b.
log[OH–].
d.
[H2O].
 

18. 
What is the pH of a 10–4 M HCl solution?
a.
4
c.
8
b.
6
d.
10
 

19. 
What is the pH of a 10–5 M KOH solution?
a.
3
c.
9
b.
5
d.
11
 

20. 
If [H3O+] = 1.7 ´ 10–3 M, what is the pH of the solution?
a.
1.81
c.
2.42
b.
2.13
d.
2.77
 

21. 
If [H3O+] = 8.26 ´ 10–5 M, what is the pH of the solution?
a.
2.161
c.
4.083
b.
3.912
d.
8.024
 

22. 
What is the pH of a solution whose hydronium ion concentration is 5.03 ´ 10–1 M?
a.
0.2984
c.
1.542
b.
0.5133
d.
5.031
 

23. 
What is the pH of a 0.027 M KOH solution?
a.
6.47
c.
12.92
b.
12.43
d.
14.11
 

24. 
What is the hydronium ion concentration of a solution whose pH is 4.12?
a.
4.4 ´ 10–8 M
c.
6.4 ´ 10–5 M
b.
5.1 ´ 10–6 M
d.
7.6 ´ 10–5 M
 

25. 
What is the hydronium ion concentration of a solution whose pH is 7.30?
a.
1.4 ´ 10–11 M
c.
5.0 ´ 10–8 M
b.
3.8 ´ 10–8 M
d.
7.1 ´ 10–6 M
 

26. 
What is the hydroxide ion concentration of a solution whose pH is 12.40?
a.
2.5 ´ 10–2 M
c.
8.9 ´ 10–2 M
b.
4.4 ´ 10–2 M
d.
1.0 ´ 10–1 M
 

27. 
Dyes with pH-sensitive colors are used as
a.
primary standards.
c.
titrants.
b.
indicators.
d.
None of the above
 

28. 
The pH range over which an indicator changes color is its
a.
equivalence point.
c.
transition interval.
b.
endpoint.
d.
pH interval.
 

29. 
Indicators are classified into three types according to
a.
their molar mass.
c.
their color.
b.
their polarity.
d.
the pH at which they change color.
 

30. 
What is the transition interval for litmus?
a.
pH 3.2–4.4
c.
pH 6.0–7.6
b.
pH 5.5–8.0
d.
pH 8.2–10.6
 

31. 
What is the transition interval for bromthymol blue?
a.
pH 3.2–4.4
c.
pH 6.0–7.6
b.
pH 5.5–8.0
d.
pH 8.2–10.6
 

32. 
What is the transition interval for phenolphthalein?
a.
pH 3.2–4.4
c.
pH 6.0–7.6
b.
pH 5.5–8.0
d.
pH 8.2–10.6
 

33. 
What is the transition interval for methyl orange?
a.
pH 3.2–4.4
c.
pH 6.0–7.6
b.
pH 5.5–8.0
d.
pH 8.2–10.6
 

34. 
Which indicator is used to study neutralizations of strong acids with strong bases?
a.
phenolphthalein
c.
bromthymol blue
b.
methyl orange
d.
None of the above
 

35. 
Which indicator is used to study neutralizations of weak acids with strong bases?
a.
phenolphthalein
c.
bromthymol blue
b.
methyl orange
d.
None of the above
 

36. 
What process measures the amount of a solution of known concentration required to react with a measured amount of a solution of unknown concentration?
a.
autoprotolysis
c.
neutralization
b.
hydrolysis
d.
titration
 

37. 
An acid-base titration involves a
a.
composition reaction.
c.
single-replacement reaction.
b.
neutralization reaction.
d.
decomposition reaction.
 

38. 
Which quantity is directly measured in a titration?
a.
mass
c.
volume
b.
concentration
d.
density
 

39. 
An acid-base titration determines the volumes of two solutions that
a.
are chemically equivalent.
c.
have equal mass.
b.
have equal molarity.
d.
have equal molality.
 

40. 
What unknown quantity can be calculated after performing a titration?
a.
volume
c.
mass
b.
concentration
d.
density
 

41. 
An acid-base titration is carried out by monitoring
a.
temperature.
c.
pressure.
b.
pH.
d.
density.
 

42. 
In an acid-base titration, equivalent quantities of hydronium ions and hydroxide ions are present
a.
at the beginning point.
c.
at the endpoint.
b.
at the midpoint.
d.
throughout the titration.
 

43. 
During an acid-base titration, a very rapid change in pH
a.
occurs when the first addition of the known solution is made.
b.
occurs when the amounts of H3O+ and OH– are nearly equivalent.
c.
occurs at several points during the titration.
d.
does not occur during titration.
 

44. 
What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration by 40.0 mL of 0.400 M NaOH?
a.
0.200 M
c.
0.320 M
b.
0.280 M
d.
0.500 M
 

45. 
What is the molarity of an HCl solution if 125 mL is neutralized in a titration by 76.0 mL of 1.22 M KOH?
a.
0.371 M
c.
0.617 M
b.
0.455 M
d.
0.742 M
 

46. 
Calculate the molarity of a Ba(OH)2 solution if 1900 mL is completely titrated by 261 mL of 0.505 M HNO3.
a.
0.0173 M
c.
0.0322 M
b.
0.0254 M
d.
0.0347 M
 

47. 
If 72.1 mL of 0.543 M H2SO4 completely titrates 39.0 mL of KOH solution, what is the molarity of the KOH solution?
a.
0.317 M
c.
1.00 M
b.
0.502 M
d.
2.01 M
 

48. 
If 114 mL of 0.008 04 M NaOH completely titrates 118 mL of H3PO4 solution, what is the molarity of the H3PO4 solution?
a.
0.002 59 M
c.
0.007 77 M
b.
0.005 18 M
d.
0.0105 M
 

49. 
What is the molarity of a Ba(OH)2 solution if 93.9 mL is completely titrated by 15.3 mL of 0.247 M H2SO4?
a.
0.0101 M
c.
0.0402 M
b.
0.0201 M
d.
0.0805 M
 

50. 
What is the molarity of an H3PO4 solution if 358 mL is completely titrated by 876 mL of 0.0102 M Ba(OH)2 solution?
a.
0.0111 M
c.
0.0250 M
b.
0.0166 M
d.
0.0333 M
 



 
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