Practice Quiz  -  Chapter 14                                       Name: __________________________


1.	Which of the following is a conjugate acid/base pair?
A)	HCl/OCl–
B)	H2SO4/SO42–
C)	NH4+/NH3
D)	H3O+/OH–
E)	more than one of these

2.	The hydrogen sulfate or bisulfate ion HSO4– can act as either an acid or a base in water solution. In which of the following equations does HSO4– act as an acid?
A)	HSO4– + H2O → H2SO4 + OH–
B)	HSO4– + H3O+ → SO3 + 2H2O
C)	HSO4– + OH– → H2SO4 + O2–
D)	HSO4– + H2O → SO42– + H3O+
E)	none of these

Use the following to answer questions 3-4:
Consider the following reactions:

a)	Al3+ + 6H2O   Al(OH2)63+
b)	Al(OH2)63+   Al(OH)(OH2)52+ + H+
c)	OCl– + H2O   HOCl + OH–
d)	CN– + H+   HCN
e)		none of these

3.	Which is associated with the definition of Ka?
A)	a
B)	b
C)	c
D)	d
E)	e

4.	Which is associated with the definition of Kb?
A)	a
B)	b
C)	c
D)	d
E)	e

5.	Using the following Ka values, indicate the correct order of base strength.

HNO2	Ka = 4.0   10–4
HF	Ka = 7.2   10–4
HCN	Ka = 6.2   10–10

A)	CN– > NO2– > F– > H2O > Cl–
B)	Cl– > H2O > F– > NO2– > CN–
C)	CN– > F– > NO2– > Cl– > H2O
D)	H2O > CN– > NO2– > F– > Cl–
E)	none of these


Use the following to answer questions 6-7:
 Consider the reaction HOCl + F–   HF + OCl–


6.	Given that Ka for HOCl is 3.5 × 10–8 and the Ka for HF is 7.2 × 10–4 (both at 25°C), which of the following is true concerning K for the above reaction at 25°C?
A)	K is greater than 1.
B)	K is less than 1.
C)	K is equal to 1.
D)	Cannot be determined with the above information.
E)	None of these (A-D).

7.	Assuming that the value for K in the above reaction is greater than 1, this means that HF is a stronger acid than HOCl.
A)	True
B)	False
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8.	The autoionization of water, as represented by the below equation, is known to be endothermic. Which of the following correctly states what occurs as the temperature of water is raised?  H2O(l) + H2O(l)   H3O+(aq) + OH–(aq)
A)	The pH of the water does not change, and the water remains neutral.
B)	The pH of the water decreases, and the water becomes more acidic.
C)	The pH of the water decreases, and the water remains neutral.
D)	The pH of the water increases, and the water becomes more acidic.
E)	The pH of the water increases and the water remains neutral.

9.	In deciding which of two acids is the stronger, one must know:
A)	the concentration of each acid solution
B)	the pH of each acid solution
C)	the equilibrium constant of each acid
D)	all of the above
E)	both A and C must be known

10.	Calculate the pH of 0.298 M HNO3(aq).
A)	0.526
B)	2.980
C)	–1.137
D)	13.702
E)	1.211

11.	Calculate the pOH of a 5.3 M solution of HCl.
A)	–0.72
B)	13.28
C)	14.72
D)	0.72
E)	–0.94

12.	What volume of water must be added to 11.0 mL of a pH 2.0 solution of HNO3 in order to change the pH to 4.0?
A)	11.0 mL
B)	89 mL
C)	109 mL
D)	1.09 × 103 mL
E)	28 mL

13.	Calculate the pH of a 0.17 M solution of HOCl, Ka = 3.5   10–8.
A)	4.11
B)	8.23
C)	9.89
D)	1.00
E)	3.77

14.	Calculate the pOH of a 0.56 M solution of acetic acid (Ka = 1.8   10–5).
A)	2.50
B)	9.00
C)	5.00
D)	11.50
E)	2.25

15.	Calculate the pH of the following aqueous solution:
	0.56 M HOCl (pKa = 7.46)
A)	10.14
B)	3.86
C)	7.71
D)	6.29
E)	none of these

16.	A solution of 2.3 M weak acid is 0.52% ionized. What is the Ka value of this acid?
A)	6.3 × 10–5
B)	1.2
C)	1.2 × 10–2
D)	5.2 × 10–3
E)	none of these


17.	Which of the following solutions contains the strongest acid?
A)	5.00 M HCN (Ka = 6.2 × 10–10)
B)	3.50 M H2C6H6O6 (Ka1 = 7.9 × 10–5, Ka2 = 1.6 × 10–12).
C)	2.50 M HC2H3O2 (Ka = 1.8 × 10–5)
D)	4.00 M HOCl (Ka = 3.5 × 10–8)
E)	1.00 M HF (Ka = 7.2 ´ 10–4)

18.	Calculate the pOH of a 0.25 M solution of Ba(OH)2.
A)	0.60
B)	0.30
C)	13.70
D)	13.40
E)	none of these

19.	Calculate the pH of a 0.86 M NH3 (Kb = 1.8   10–5) solution.
A)	2.41
B)	9.19
C)	4.81
D)	0.86
E)	11.59

20.	What is the equilibrium concentration of PO43– in a 0.819 M solution of H3PO4(aq)? (Ka1 = 7.5 × 10–3, Ka2 = 6.2 × 10–8, Ka3 = 4.8 × 10–13)
A)	7.5 × 10–2 M
B)	2.3 × 10–4 M
C)	4.8 × 10–13 M
D)	6.3 × 10–7 M
E)	6.2 × 10–8 M

Use the following to answer question 21:
Select the answer that best describes an aqueous solution made from each of the following substances:


21.	solid sodium nitrate (NaNO3)
A)	acidic
B)	basic
C)	neutral
D)	cannot tell
E)	none of these (A-D)
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22.	Calculate the pH of the following aqueous solution:
	0.55 M NaF (pKa for HF = 3.14)
A)	5.56
B)	2.88
C)	8.44
D)	11.12
E)	none of these

23.	A 0.409 M solution of the salt NaA has a pH of 8.40. Calculate the Ka value of the acid HA.
A)	1.5 × 10–11
B)	1.6 × 10–9
C)	6.5 × 10–4
D)	2.6 × 102
E)	none of these

24.	Which of the following species cannot act as a Lewis acid?
A)	K+
B)	Mg2+
C)	Al3+
D)	H+
E)	H–

25.	Consider the following reaction:
AgBr(s) + 2CN–(aq)   Ag(CN)2–(aq) + Br–(aq)
The species that are acting as a Lewis acid and Lewis base, respectively, are
A)	AgBr and Ag(CN)2–
B)	Ag(CN)2– and Ag+
C)	Ag+ and Br–
D)	Br– and CN–
E)	Ag+ and CN–


Answers:

1.	C
2.	D
3.	B
4.	C
5.	A
6.	B
7.	B
8.	C
9.	C
10.	A
11.	C
12.	D
13.	A
14.	D
15.	B
16.	A
17.	E
18.	B
19.	E
20.	C
21.	C
22.	C
23.	C
24.	E
25.	E