Determine the pH in a 0.667 M NaOH solution. Group of answer choices0.12 0.18 14.18 13.88 13.82 Question 22 pts What is the pH of a buffer solution that is 0.192 M in lactic acid and 0.155 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4. Group of answer choices3.94 14.09 10.24 3.76 5.48 Question 32 pts Determine the pH of a 0.22 M NaF solution at 25°C. The Ka of HF is 3.5 × 10-5. Group of answer choices5.10 11.44 10.20 8.90 2.56 Question 42 pts Which of the following compounds solubility will NOT be affected by a low pH in solution? Group of answer choicesBaCO3 AgCl CuS Mg(OH)2 BaF2 Question 52 pts Determine the molar solubility of CaSO4 in a solution containing 0.060 M Na2SO4. Ksp (CaSO4) = 2.4 × 10-5. Group of answer choices5.8 × 10-10 M 4.0 × 10-4 M 0.30 M 1.4 × 10-6 M 4.9 × 10-3 M Question 62 pts Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion. Group of answer choices4.15 × 10-4 7.05 2.41 × 10-11 10.62 3.38 Question 72 pts Identify the base that is in baking soda. Group of answer choicesNaHCO3 LiOH KHCO3 RbOH Li2CO3 Question 82 pts A 25.0 mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of butanoic acid is 1.5 × 10-5. Group of answer choices8.85 11.82 9.18 7.10 4.82 Question 92 pts Determine the [H3O+] concentration for a 0.200 M solution of HCl. Group of answer choices1.00 × 10-1 M 4.00 × 10-1 M 2.50 × 10 -14 M 1.25 × 10-14 M 2.00 × 10-1 M Flag question: Question 10 Question 102 pts A ligand is a molecule or ion that acts as a Group of answer choicesLewis base. Brønsted-Lowry base. conjugate acid. Arrhenius base. Lewis acid. Flag question: Question 11 Question 112 pts Calculate the pH of a solution that is 0.112 M in sodium formate (NaHCO2) and in formic acid The Ka of formic acid is 1.77 × 10-4. Group of answer choices10.63 5.073 3.369 14.38 4.121 Flag question: Question 12 Question 122 pts A 700.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M CsOH. Determine the pH of the solution after the addition of 350.0 mL of CsOH. Group of answer choices1.52 0.68 2.35 12.48 3.22 Flag question: Question 13 Question 132 pts What is the pH of a 0.020 M Ba(OH)2 solution? Group of answer choices1.70 1.40 12.60 13.20 12.30 Flag question: Question 14 Question 142 pts A solution contains Fe2+, Ba2+, Ag+, NH4+, and Cd2+. Identify the soluble compound after the addition of 6 M HCl; then H2S and 0.2 M HCl; then OH- to a pH of 8; and then (NH4)2HPO4 with NH3. Group of answer choicesBa3(PO4)2 CdS NH4Cl FeS AgCl Flag question: Question 15 Question 152 pts Which of the following is a Lewis acid? Group of answer choicesAlBr3 CHBr3 NH3 CCl4 None of the above is a Lewis acid. Flag question: Question 16 Question 162 pts Calculate the Ksp for hydroxide if the solubility of Mn(OH.

1. Determine the pH in a 0.667 M NaOH solution.
Group of answer choices0.12
0.18
14.18
13.88
13.82
Question 22
pts
What is the pH of a buffer solution that is 0.192 M in lactic acid
and 0.155 M in sodium lactate? The Ka of lactic acid is 1.4 ×
10-4.
Group of answer choices3.94
14.09
10.24
3.76
5.48

2. Question 32
pts
Determine the pH of a 0.22 M NaF solution at 25°C. The Ka of
HF is 3.5 × 10-5.
Group of answer choices5.10
11.44
10.20
8.90
2.56
Question 42
pts
Which of the following compounds solubility will NOT be
affected by a low pH in solution?
Group of answer choicesBaCO3
AgCl
CuS
Mg(OH)2

3. BaF2
Question 52
pts
Determine the molar solubility of CaSO4 in a solution
containing 0.060 M Na2SO4. Ksp (CaSO4) = 2.4 × 10-5.
Group of answer choices5.8 × 10-10 M
4.0 × 10-4 M
0.30 M
1.4 × 10-6 M
4.9 × 10-3 M
Question 62
pts
Calculate the pH for an aqueous solution of pyridine that
contains
hydroxide ion.
Group of answer choices4.15 × 10-4

4. 7.05
2.41 × 10-11
10.62
3.38
Question 72
pts
Identify the base that is in baking soda.
Group of answer choicesNaHCO3
LiOH
KHCO3
RbOH
Li2CO3
Question 82
pts
A 25.0 mL sample of 0.150 M butanoic acid is titrated with a
0.150 M NaOH solution. What is the pH at the equivalence
point? The Ka of butanoic acid is 1.5 × 10-5.

5. Group of answer choices8.85
11.82
9.18
7.10
4.82
Question 92
pts
Determine the [H3O+] concentration for a 0.200 M solution of
HCl.
Group of answer choices1.00 × 10-1 M
4.00 × 10-1 M
2.50 × 10 -14 M
1.25 × 10-14 M
2.00 × 10-1 M
Flag question: Question 10
Question 102

6. pts
A ligand is a molecule or ion that acts as a
Group of answer choicesLewis base.
Brønsted-Lowry base.
conjugate acid.
Arrhenius base.
Lewis acid.
Flag question: Question 11
Question 112
pts
Calculate the pH of a solution that is 0.112 M in sodium
formate (NaHCO2) and
in formic acid
The Ka of formic acid is 1.77 × 10-4.
Group of answer choices10.63
5.073
3.369
14.38

7. 4.121
Flag question: Question 12
Question 122
pts
A 700.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M
CsOH. Determine the pH of the solution after the addition of
350.0 mL of CsOH.
Group of answer choices1.52
0.68
2.35
12.48
3.22
Flag question: Question 13
Question 132
pts
What is the pH of a 0.020 M Ba(OH)2 solution?
Group of answer choices1.70

8. 1.40
12.60
13.20
12.30
Flag question: Question 14
Question 142
pts
A solution contains Fe2+, Ba2+, Ag+, NH4+, and Cd2+.
Identify the soluble compound after the addition of 6 M HCl;
then H2S and 0.2 M HCl; then OH- to a pH of 8; and then
(NH4)2HPO4 with NH3.
Group of answer choicesBa3(PO4)2
CdS
NH4Cl
FeS
AgCl
Flag question: Question 15
Question 152

9. pts
Which of the following is a Lewis acid?
Group of answer choicesAlBr3
CHBr3
NH3
CCl4
None of the above is a Lewis acid.
Flag question: Question 16
Question 162
pts
Calculate the Ksp for hydroxide if the solubility of Mn(OH)2 in
pure water is 7.18 × 10-1 g/L.
Group of answer choices2.10 × 10-6
5.50 × 10-11
8.07 × 10-3
7.18 × 10-1
5.25 × 10-7

10. Flag question: Question 17
Question 172
pts
What is the hydronium ion concentration of a 0.100 M
hypochlorous acid solution with
The equation for the dissociation of hypochlorous acid is:
HOCl(
aq
) + H2O(
l
) ⇌ H3O+(
aq
) + OCl-(
aq
)
Group of answer choices5.9 × 10-4 M
1.9 × 10-5 M
1.9 × 10-4 M
5.9 × 10-5 M
Flag question: Question 18
Question 182

11. pts
What is the pH of a solution made by mixing 29.00 mL of 0.10
M acetic acid with 29.00 mL of 0.10 M KOH? Assume that the
volumes of the solutions are additive. Ka =
for CH3CO2H.
Group of answer choices7.00
5.28
6.22
10.02
8.72
Flag question: Question 19
Question 192
pts
Calculate the pH of a solution formed by mixing 150.0 mL of
0.20 M HClO with 300.0 mL of 0.30 M CsClO. The Ka for
HClO is 2.9 × 10-8.
Group of answer choices6.46
5.99
7.06

12. 7.54
8.01
Flag question: Question 20
Question 202
pts
Calculate the pH of a 0.16 M carbonic acid solution, H2CO3(
aq
), that has the stepwise dissociation constants
K
a1 = 4.3 × 10-7 and
K
a2 = 5.6 × 10-11.
Group of answer choices3.58
10.25
6.37
0.80
Flag question: Question 21
Question 212
pts

13. What is the hydroxide ion concentration of a NaOH solution
that has a pH of 12.20?
Group of answer choices12.20 M
1.58 × 10-2 M
1.80 M
7.20
6.31 × 10-13 M
Flag question: Question 22
Question 222
pts
Calculate the pH of a solution that is 0.322 M in nitrous acid
(HNO2) and 0.178 M in potassium nitrite (KNO2). The acid
dissociation constant of nitrous acid is 4.50 × 10-4.
Group of answer choices3.607
10.91
4.554
14.26
3.093

14. Flag question: Question 23
Question 232
pts
What is the pH of the resulting solution if 45.00 mL of 0.10 M
acetic acid is added to 10.00 mL of 0.10 M KOH? Assume that
the volumes of the solutions are additive. Ka = 1.8 × 10-5 for
CH3CO2H
Group of answer choices6.62
5.29
9.80
4.20
8.71
Flag question: Question 24
Question 242
pts
Place the following in order of
increasing
acid strength.
HBrO2HBrO3HBrOHBrO4

15. Group of answer choicesHBrO4 < HBrO2 < HBrO3 < HBrO
HBrO < HBrO4 < HBrO3 < HBrO2
HBrO2 < HBrO4 < HBrO < HBrO3
HBrO < HBrO2 < HBrO3 < HBrO4
HBrO2 < HBrO3 < HBrO4 < HBrO
Flag question: Question 25
Question 252
pts
Determine the pH of a 0.00444 M HClO4 solution.
Group of answer choices1.353
2.353
12.647
11.647
5.824
Flag question: Question 26
Question 262

16. pts
A 6.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a
pH of ________.
Group of answer choices5.6 × 10-13
12.08
1.92
11.78
1.2 × 10-2
Flag question: Question 27
Question 272
pts
An aqueous solution at 25.0°C contains [H+] = 0.099 M. What
is the pH of the solution?
Group of answer choices0.0990
1.00
13.0
-1.00

17. 1.20 × 10-13
Flag question: Question 28
Question 282
pts
Calculate the molar solubility of thallium chloride in 0.0.25 M
NaCl at 25°C. Ksp for TlCl is
Group of answer choices8.2 × 10-3 M
6.8 × 10-4 M
1.7 × 10-5 M
1.3 × 10-2 M
Flag question: Question 29
Question 292
pts
Calculate the pH for an aqueous hydroiodic acid solution that
contains
hydronium ion.
Group of answer choices11.50
2.50

18. 12.50
3.17 × 10-12
3.15 × 10-3
Flag question: Question 30
Question 302
pts
Describe what happens at high pH for aluminum hydroxide.
Group of answer choicesAl(H2O)23+ precipitates.
Al precipitates.
Al dissolves.
Al(H2O)2(OH)4- dissolves.
Al(OH)5 precipitates.
Flag question: Question 31
Question 312
pts
Which of the following acids (listed with Ka values) and their
conjugate base should be used to form a buffer with a pH of

19. 2.34?
Group of answer choicesHClO2, Ka = 1.1 × 10-2
HIO, Ka = 2.3 × 10-10
HCN, Ka = 4.9 × 10-10
C6H5OH, Ka = 1.3 × 10-10
HN3, Ka = 2.5 × 10-5
Flag question: Question 32
Question 322
pts
How many milliliters of 0.0991 M LiOH are required to titrate
25.0 mL of
to the equivalence point?
Group of answer choices0.208
4.58
29.5
21.2
0.333

20. Flag question: Question 33
Question 332
pts
A solution contains Ba2+, Hg2+, Ag+, NH4+, and Fe2+.
Identify the precipitate after the addition of 6 M HCl.
Group of answer choicesHgS
Ba3(PO4)2
FeS
AgCl
NH4Cl
Flag question: Question 34
Question 342
pts
Identify the diprotic acid.
Group of answer choicesCH3COOH
HNO3
H2SO3

21. HClO4
HF
Flag question: Question 35
Question 352
pts
Find the percent ionization of a 0.337 M HF solution. The Ka
for HF is 3.5 × 10-4.
Group of answer choices4.7%
1.2 × 10-2%
3.2%
1.1%
3.5 × 10-2%
Flag question: Question 36
Question 362
pts
Identify the
weak
monoprotic acid.

22. Group of answer choicesH2CO3
NaBr
HF
HNO3
LiOH
Flag question: Question 37
Question 372
pts
Determine the pH of a 0.141 M RbOH solution at 25°C.
Group of answer choices13.86
13.15
0.141
0.851
0.88
Flag question: Question 38
Question 382

23. pts
Calculate the pH of a solution that contains 7.8 × 10-6 M OH⁻
at 25°C.
Group of answer choices8.89
12.72
1.28
5.11
9.64
Flag question: Question 39
Question 392
pts
What is the pH of a 0.300 M NH3 solution that has
K
b = 1.8 × 10-5? The equation for the dissociation of NH3 is:
NH3(
aq
) + H2O(
l
) ⇌ NH4+(
aq
) + OH-(
aq

24. )
Group of answer choices10.89
2.11
11.37
6.22
2.63
Flag question: Question 40
Question 402
pts
A 150.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M
LiOH. Determine the pH of the solution after the addition of
45.0 mL of LiOH.
Group of answer choices1.21
1.12
0.86
2.00
2.86

25. Flag question: Question 41
Question 412
pts
Formic acid (HCO2H, Ka = 1.8 × 10-4) is the principal
component in the venom of stinging ants. What is the molarity
of a formic acid solution if 25.00 mL of the formic acid solution
requires 74.80 mL of 0.0567 M NaOH to reach the equivalence
point?
Group of answer choices0.170 M
0.0375 M
0.0190 M
0.0567 M
0.0134 M
Flag question: Question 42
Question 422
pts
Which of the following acids (listed with pKa values) and their
conjugate base should be used to form a buffer with a pH of
8.10?
Group of answer choicesHC7H5O2, pKa = 4.19

26. HF, pKa = 3.46
HClO, pKa = 7.54
H2SO3, pKa = 1.77
HClO2, pKa = 1.96
Flag question: Question 43
Question 432
pts
Calculate the pH of a buffer that is 1.26 M HClO and 0.079 M
NaClO. The Ka for HClO is 2.9 × 10-8.
Group of answer choices7.46
6.67
7.74
7.54
6.34
Flag question: Question 44
Question 442
pts

27. A 550.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M
KOH. Determine the pH of the solution after the addition of
550.0 mL of KOH.
Group of answer choices1.35
12.85
12.65
13.13
0.87
Flag question: Question 45
Question 452
pts
Calculate the pH of a buffer that is 0.080 M HF and 0.040 M
NaF. The Ka for HF is 3.5 × 10-4.
Group of answer choices4.86
2.06
3.56
3.76
3.16

28. Flag question: Question 46
Question 462
pts
Which one of the following salts, when dissolved in water,
produces the solution with the
highest
pH?
Group of answer choicesCsCl
CsI
CsF
CsBr
Flag question: Question 47
Question 472
pts
What is the pH at the equivalence point of a weak base-strong
acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.40
M HCl to reach the equivalence point? Ka = 3.0 × 10-8 for
HOCl.
Group of answer choices2.10

29. 0.40
3.23
3.76
4.08
Flag question: Question 48
Question 482
pts
A solution contains Zn2+, Hg2+, Ag+, NH4+, and Ba2+.
Identify the precipitate after the addition of 6 M HCl, then H2S
and 0.2 M HCl.
Group of answer choicesBa3(PO4)2
ZnS
NH4Br
AgCl
HgS
Flag question: Question 49
Question 492

30. pts
A 220.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH.
Determine the pH of the solution after the addition of 440.0 mL
of NaOH. The Ka of HF is 3.5 × 10-4.
Group of answer choices3.46
8.14
7.00
9.62
10.54
Flag question: Question 50
Question 502
pts
The
largest
change in pH for an effective buffer occurs when the base is
how many times as concentrated as the acid?
Group of answer choices6
20
5

31. 40
10