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CHEM 1120 Test 1 - Spring 2005: Calculating pH Values and Equilibrium Constants, Exams of Chemistry

Roane State Community CollegeChemistry

A chemistry test consisting of 20 multiple-choice questions. The questions cover various topics such as calculating ph values of different solutions, identifying spectator ions, and determining equilibrium constants. Students are required to use the given equilibrium constants to answer the questions.

Typology: Exams

Pre 2010

Uploaded on 08/19/2009

koofers-user-dah
koofers-user-dah 🇺🇸

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CHEM 1120 test 1 - Spring 2005 Page 1
Circle the correct answer on the answer sheet. Use the equilibrium constants on the sheet
attached.
1. Calculate the pH of a 0.025
M
solution of HClO
4
.
a. 1.00 b. 1.60 c. 7.00 d. 12.40 e. 13.70
2. Calculate the pH of a 0.50
M
solution of KOH.
a. 1.00 b. 1.60 c. 7.00 d. 12.40 e. 13.70
3. Calculate the pH of a 0.025
M
solution of KBrO
3.
a. 1.00 b. 1.60 c. 7.00 d. 12.40 e. 13.70
4. Calculate the pH of a 0.20
M
solution of HNO
2
a. 0.70 b. 1.05 c. 2.05 d. 11.95 e. 12.95
5. Calculate the pH of a 1.0
M
solution of CH
3
NH
2
.
a. 1.51 b. 2.34 c. 7.00 d. 11.49 e. 12.49
6. Calculate the pH of a solution in contact with solid Mg(OH)
2
. No other ions are present in
the water.
a. 1.44 b. 3.84 c. 7.00 d. 10.15 e. 14.00
7. What is the molar solubility of Cu
2
S?
a. 1.7 × 10
-16
b. 4.2 × 10
-16
c. 1.0 × 10
-5
d. 2.0 × 10
-47
e. 2.7 × 10
-16
8. Calculate the pH of a mixture solution of 0.20
M
NH
3
and 0.20
M
NH
4
NO
3
.
a. 2.35 b. 4.77 c. 7.00 d. 9.23 e. 11.23
pf3
pf4
pf5

Partial preview of the text

Download CHEM 1120 Test 1 - Spring 2005: Calculating pH Values and Equilibrium Constants and more Exams Chemistry in PDF only on Docsity!

Circle the correct answer on the answer sheet. Use the equilibrium constants on the sheet attached.

  1. Calculate the pH of a 0.025 M solution of HClO 4. a. 1.00 b. 1.60 c. 7.00 d. 12.40 e. 13.
  2. Calculate the pH of a 0.50 M solution of KOH. a. 1.00 b. 1.60 c. 7.00 d. 12.40 e. 13.
  3. Calculate the pH of a 0.025 M solution of KBrO3. a. 1.00 b. 1.60 c. 7.00 d. 12.40 e. 13.
  4. Calculate the pH of a 0.20 M solution of HNO 2 a. 0.70 b. 1.05 c. 2.05 d. 11.95 e. 12.
  5. Calculate the pH of a 1.0 M solution of CH 3 NH 2. a. 1.51 b. 2.34 c. 7.00 d. 11.49 e. 12.
  6. Calculate the pH of a solution in contact with solid Mg(OH) 2. No other ions are present in the water. a. 1.44 b. 3.84 c. 7.00 d. 10.15 e. 14.
  7. What is the molar solubility of Cu 2 S? a. 1.7 × 10-16^ b. 4.2 × 10-16^ c. 1.0 × 10-5^ d. 2.0 × 10-47^ e. 2.7 × 10-
  8. Calculate the pH of a mixture solution of 0.20 M NH 3 and 0.20 M NH 4 NO 3. a. 2.35 b. 4.77 c. 7.00 d. 9.23 e. 11.
  1. Calculate the pH of a mixture solution of 0.50 M NaF and 0.10 M HF. a. 2.50 b. 3.20 c. 3.90 d. 10.80 e. 11.
  2. Calculate the pH of a 0.50 M solution of KF. a. 3.54 b. 5.40 c. 5.55 d. 8.45 e. 8.
  3. Calculate the pH of a 0.20 M solution of NH 3 ClO 3. a. 4.62 b. 4.97 c. 9.03 d. 9.38 e. 10.
  4. Calculate the pH of a solution created by mixing 100 mL of 0.100 M NaOH with 200 mL of 0.100 M CH 3 COOH. a. 3.45 b. 4.77 c. 7.00 d. 9.23 e. 12.
  5. Calculate the pH of a solution created by mixing 100 mL of 0.100 M HBr and 100 mL of 0.100 M NH 3. a. 3.24 b. 4.62 c. 5.27 d. 8.73 e. 9.
  6. A solution of Co(NH 3 ) 6 Cl 3 is at equilibrium with Co3+^ and NH 3 (aq). The concentration of the NH 3 is 0.50 M and the Co(NH 3 ) 6 3+^ ion concentration is 0.0010 M. Calculate the concentration of the Co3+^ ion. (Kd(Co(NH 3 ) 6 3+) = 1.2 × 10-5^ ) a. 2.6 × 10-10^ M b. 7.68 × 10–7^ M c. 3.0 × 10-2^ M d. 4.3 × 10-2^ M e. 0.20 M
  7. A solution of Co(NH 3 ) 6 Cl 3 is made up to be 0.10 M. Calculate the resultant concentration of the Co3+^ ion. (Kd(Co(NH 3 ) 6 3+) = 1.2 × 10-5^ ) a. 3.0 × 10-2^ M b. 4.3 × 10-2^ M c. 0.20 M d. 7.68 × 10–7^ M e. 2.6 × 10-10^ M
  8. Which of the following ions is a spectator anion in an acid-base reaction? a. NO 2 –^ b. SO 3 2–^ c. F–^ d. Na+^ e. IO 3 –

ANSWER SHEET

NAME__________________________________________________________________

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KEY

1.b 2.e 3.c 4.c 5.e 6.d 7.a 8.d 9.c 10.d 11.b 12.b 13.c 14.b 15.a 16.e 17.b 18.c 19.d 20.c