C12 Practice Exam 2 (version with no time limit) - CHEM 1312, section 11651, Summer 1 2025 | WebAssign
7/17/25, 9:02 PM
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CHEM 1312, section 11651, Summer 1 2025
INSTRUCTOR
C12 Practice Exam 2 (version with no time limit) (Practice)
Arkadiusz Czader
University of Houston, TX
Due Date: FRI, AUG 22, 2025 11:59 PM CDT
Current Score: – / 22 POINTS | 0.0 %
Submissions Used: 0 / 4
Scoring and Assignment Information
QUESTION
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POINTS
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Instructions
This exam is timed, and the countdown timer should appear in the upper left of the page. Each question must be submitted before your time
expires.
The periodic table and a simple scientific calculator are available below.
▸ Periodic Table and Physical Constants
▸ Chemical Calculator
Open tab with Chemistry Calculator or with Periodic Table and Physical Constants
Assignment Submission
For this assignment, you submit the entire assignment.
Assignment Scoring
Your best submission for each entire question is used for your score.
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Page 1 of 7
C12 Practice Exam 2 (version with no time limit) - CHEM 1312, section 11651, Summer 1 2025 | WebAssign
1.
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7/17/25, 9:02 PM
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Given the following acids and pK a values,
HClO 2 (pK a = 2.00)
CCl 3COOH (pK a = 0.52)
HIO 3 =(pK a 0.77)
HBrO 2 (pK a = 4.69)
HN 3 (pK a = 4.72)
which of the compounds listed below is the strongest base?
ClO 2 BrO 2 IO 3 N3CCl 3COO -
2.
[– / 1 Points]
What is the pH of a solution prepared by dissolving 0.075 mol of Ba(OH) 2 in water to give 455 mL of solution?
13.52
12.92
13.22
0.48
0.78
3.
[– / 1 Points]
Give the conjugate base of H 3S +.
Formatting counts; use superscripts and subscripts if needed.
4.
[– / 1 Points]
At 25°C , what is the [OH -] in a solution that has a pH = 10.53?
M
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C12 Practice Exam 2 (version with no time limit) - CHEM 1312, section 11651, Summer 1 2025 | WebAssign
5.
[– / 1 Points]
The K a of HCN is 5.0
7/17/25, 9:02 PM
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10 -10. What is the pH of 0.050 M HCN?
Between 3.5 and 4.5
Between 5.0 and 5.5
Between 4.5 and 5.0
Between 8.5 and 9.5
Between 9.5 and 10.5
6.
[– / 1 Points]
Calculate the pH of a 0.30 M solution of aniline (C 6H 5NH 2), with a K b = 3.8
10 -10.
9.03
4.97
9.42
2.55
11.45
7.
[– / 1 Points]
At a certain temperature, the percent dissociation (ionization) of chlorous acid, HClO 2, in a 1.53 M solution water is 10.0%. Calculate the value of K a for
chlorous acid at this temperature.
8.
2.3
10 -2
1.0
10 -1
1.5
10 -1
7.0
10 -3
1.7
10 -2
[– / 1 Points]
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Rank the following 0.10 M solutions in order of increasing pH:
HCl, LiCl, NH 4Cl, NH 3.
Lowest pH (left) to highest pH (right):
---Select---
< ---Select---
< ---Select---
< ---Select---
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C12 Practice Exam 2 (version with no time limit) - CHEM 1312, section 11651, Summer 1 2025 | WebAssign
[– / 1 Points]
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Choose the stronger acid in each of the following pairs.
Formatting counts; remember to use subscripts as needed.
(a)
H 3As or H 2Se
The stronger acid is:
H 3As
H 2Se
(b)
HClO or HIO
The stronger acid is:
HClO
HIO
[– / 1 Points]
10.
Determine whether aqueous solutions of the following salts are acidic, basic, or neutral.
(a) CrCl 3
acidic
basic
neutral
(b) NaNO 3
acidic
basic
neutral
†
11.
[– / 1 Points]
Over the course of a titration, 17.5 mL 0.0438 M sodium hydroxide (NaOH), a strong base, is added to 109.5 mL 0.0586 M potassium hydrogen phthalate
(KHP), a monoprotic weak acid. What is the concentration of potassium sodium phthalate (KNaP) in the resulting solution?
M KNaP
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Page 4 of 7
C12 Practice Exam 2 (version with no time limit) - CHEM 1312, section 11651, Summer 1 2025 | WebAssign
12.
[– / 1 Points]
7/17/25, 9:02 PM
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A buffer is prepared with concentrations of [H 2PO 4 -] = 0.100 M and [HPO 4 2-] = 0.100 M. The second dissociation constant of phosphoric acid is K a2 is
6.21 ✕ 10 −8.
If 2.97 x 10 -3 moles of KOH are added to 0.100 L of this buffer, what is the resulting pH?
13.
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What will happen if a small amount of sodium hydroxide is added to a 0.1 M ideal buffer based on HF?
The percent ionization of HF will increase.
The percent ionization of HF will decrease.
The percent ionization of HF will remain unchanged.
K a for HF will increase.
K a for HF will decrease.
14.
[– / 1 Points]
Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.060 M HCl.
K a of HF = 7.24 ✕ 10 −4
2.96
3.14
3.32
2.92
3.36
15.
[– / 1 Points]
Aniline (C 6H 5NH 2 ) has a K b = 3.8 ✕ 10 −10 If 100.0 mL of a 0.5000 M aqueous aniline solution is mixed with 100.0 mL of 0.5000 M aqueous hydrochloric
acid, the resulting solution will have a pH _____.
=7
<7
>7
Cannot be predicted from the information given
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C12 Practice Exam 2 (version with no time limit) - CHEM 1312, section 11651, Summer 1 2025 | WebAssign
16.
[– / 1 Points]
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Calculate the pH of a 0.50 M solution of sodium acetate (NaCH 3COO)
Given:K a of acetic acid (CH 3COOH ) = 1.8 ✕ 10 −5.
9.22
4.78
9.26
11.48
2.52
17.
[– / 1 Points]
Calculate the pH of a solution prepared by dissolving 0.151 mol of NH 3 and 0.160 mol of NH 4Cl in water sufficient to yield 1.00 L of solution. The base
dissociation constant of ammonia at 25°C is K b = 1.77 ✕ 10 −5.
18.
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At 25 °C the solubility of lead(II) iodide, PbI 2, is 1.52 ✕ 10 −3 mol/L. Calculate the value of K sp at this temperature.
19.
[– / 1 Points]
The K sp of AgCl at 25°C is 1.6 ✕ 10 −10. Consider a solution that is 1.0 ✕ 10 −4 M CaCl 2 and 1.0 ✕ 10 −6 M AgNO 3.
Q > K sp and a precipitate will form.
Q > K sp and a precipitate will not form.
Q < K sp and a precipitate will not form.
Q < K sp and a precipitate will form.
The solution is saturated.
20.
[– / 1 Points]
The solubility of calcium sulfate, CaSO 4, at a given temperature is 0.07850 g/L. Calculate the K sp at this temperature.
Given: calcium sulfate molar mass = 136.2 g/mol.
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C12 Practice Exam 2 (version with no time limit) - CHEM 1312, section 11651, Summer 1 2025 | WebAssign
21.
7/17/25, 9:02 PM
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What is the molar solubility of CaF 2 , assume K sp = 4.0 ✕ 10 −11 in 0.030 M NaF?
4.4 ✕ 10 −8
6.3 ✕ 10 −6
4.0 ✕ 10 −11
3.0 ✕ 10 −2
1.1 ✕ 10 −8
22.
[– / 1 Points]
Which of the following compounds will not have a different solubility with a change in pH?
AgF
Ca 3(PO 4) 2
SrCO 3
CuBr
CuS
23.
[– / 1 Points]
The K sp of AgCl is 1.61 ✕ 10 −10. What is the solubility of AgCl in a solution of 0.0869 M AlCl 3?
Assume that AlCl 3 completely dissociates into its constituent ions in solution.
M
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