A buffer is prepared by dissolving 4.00 g benzoic acid (C6H5COOH, Ka =
6.3 x 10-5) and 4.00 g sodium benzoate (C6H5COONa) in enough water to
prepare 1.00 L of solution. Calculate the pH of this buffer.
A)
4.13
B)
4.20
C)
4.27
D)
4.40
E)
5.05
Calculate the [NH3]/[NH4+] ratio in an ammonia-ammonium chloride
buffer with a pH of 9.00. (Kb for NH3 = 1.8 x 10-5)
A)
0.56/1.00
B)
0.74/1.00
C)
0.86/1.00
D)
1.12/1.00
E)
1.30/1.00
What is the pH of a buffer prepared by adding 180 mL of 0.100 M NaOH
to 200 mL of 0.100 M acetic acid? (Ka for CH3COOH = 1.8 x 10-5)
A)
3.79
B)
4.34
C)
4.74
D)
5.04
E)
5.70
Consider the titration of 50.00 mL of 0.1000 M HBr with 0.1000 M KOH.
Calculate the pH after 49.00 mL of the base has been added to the 50.00
mL of HBr.
A)
2.0
B)
3.0
C)
4.0
D)
6.0
E)
7.0
What is the optimum pH of a sodium formate/formic acid buffer? (Ka =
1.7 x 10-4)
A)
7.0
B)
6.2
C)
3.8
D)
3.0
E)
1.7
Given that the solubility of Ag2CrO4 is 0.0287 g/L, what is the value of its
Ksp?
A)
Ksp = 3.9 x 10-17
B)
Ksp = 6.5 x 10-13
C)
Ksp = 8.7 x 10-5
D)
Ksp = 7.5 x 10-9
E)
Ksp = 2.6 x 10-12
The solubility of AlF3 is 6.7 g AlF3 per liter of solution. What is the value
of the solubility product constant for AlF3?
A)
1.9 x 10-2
B)
6.0 x 10-3
C)
1.1 x 10-3
D)
4.0 x 10-4
E)
4.1 x 10-5
How many grams of AgCl will dissolve in 1.0 L of water? (Ksp for AgCl =
1.7 x 10-10)
A)
1.2 x 10-12 g
B)
2.4 x 10-8 g
C)
4.5 x 10-5 g
D)
1.8 x 10-3 g
E)
1.4 x 10-2 g
Calculate the pH of a solution necessary to just begin the precipitation
of Mg(OH)2 when [Mg2+] = 0.001 M. (Ksp for Mg(OH)2 = 1.2 x 10-11)
A)
11
B)
10
C)
9
D)
8
E)
4
Calculate the pH of a saturated solution of Mg(OH)2 (Ksp for Mg(OH)2 =
1.2 x 10-11)
A)
3.5
B)
10.2
C)
10.5
D)
11.0
E)
11.3
A buffer is prepared by dissolving 4.00 g benzoic acid (C6H5COOH, Ka =
6.3 x 10-5) and 4.00 g sodium benzoate (C6H5COONa) in enough water to
prepare 1.00 L of solution. Calculate the pH of this buffer.
A)
4.13
B)
4.20
C)
4.27
D)
4.40
E)
5.05
Calculate the [NH3]/[NH4+] ratio in an ammonia-ammonium chloride
buffer with a pH of 9.00. (Kb for NH3 = 1.8 x 10-5)
A)
0.56/1.00
B)
0.74/1.00
C)
0.86/1.00
D)
1.12/1.00
E)
1.30/1.00
What is the pH of a buffer prepared by adding 180 mL of 0.100 M NaOH
to 200 mL of 0.100 M acetic acid? (Ka for CH3COOH = 1.8 x 10-5)
A)
3.79
B)
4.34
C)
4.74
D)
5.04
E)
5.70
Consider the titration of 50.00 mL of 0.1000 M HBr with 0.1000 M KOH.
Calculate the pH after 49.00 mL of the base has been added to the 50.00
mL of HBr.
A)
2.0
B)
3.0
C)
4.0
D)
6.0
E)
7.0
What is the optimum pH of a sodium formate/formic acid buffer? (Ka =
1.7 x 10-4)
A)
7.0
B)
6.2
C)
3.8
D)
3.0
E)
1.7
Given that the solubility of Ag2CrO4 is 0.0287 g/L, what is the value of its
Ksp?
A)
Ksp = 3.9 x 10-17
B)
Ksp = 6.5 x 10-13
C)
Ksp = 8.7 x 10-5
D)
Ksp = 7.5 x 10-9
E)
Ksp = 2.6 x 10-12
The solubility of AlF3 is 6.7 g AlF3 per liter of solution. What is the value
of the solubility product constant for AlF3?
A)
1.9 x 10-2
B)
6.0 x 10-3
C)
1.1 x 10-3
D)
4.0 x 10-4
E)
4.1 x 10-5
How many grams of AgCl will dissolve in 1.0 L of water? (Ksp for AgCl =
1.7 x 10-10)
A)
1.2 x 10-12 g
B)
2.4 x 10-8 g
C)
4.5 x 10-5 g
D)
1.8 x 10-3 g
E)
1.4 x 10-2 g
Calculate the pH of a solution necessary to just begin the precipitation
of Mg(OH)2 when [Mg2+] = 0.001 M. (Ksp for Mg(OH)2 = 1.2 x 10-11)
A)
11
B)
10
C)
9
D)
8
E)
4
Calculate the pH of a saturated solution of Mg(OH)2 (Ksp for Mg(OH)2 =
1.2 x 10-11)
A)
3.5
B)
10.2
C)
10.5
D)
11.0
E)
11.3