Livingston Public Schools



Chapter 4: Practice Test

Chemical Reactions/Solutions/ Stoichiometry

Multiple Choice

1. How many grams of NaCl are contained in 350. mL of a 0.250 M solution of sodium chloride?

a) 41.7 g c) 14.6 g e) none of these

b) 5.11 g d) 87.5 g

2. The molarity of Cl- available in 110. mL of a solution containing 5.55 g of CaCl2 is:

a) 0.00550 M c) 0.668 M e) 50.5 M

b) 0.455 M d) 0.909 M

3. A 51.24 g sample of Ba(OH)2 is dissolved in enough water to make 1.20 liters of solution. How many mL is this solution must be diluted with water in order to make 1.00 liter of 0.100 M Ba(OH)2?

a) 400 mL c) 278 mL e) none of these

b) 333 mL d) 1.20 X 103 mL

4. How many grams of NaOH are contained in 5.0 X 102 mL of a 0.80 M sodium hydroxide solution?

a) 16 g c) 20. g e) none of these

b) 80. g d) 64 g

5. 25.0 mL of 0.20 M K2SO4 is added to 50.0 mL of 0.40 M KOH. Calculate the concentration of K+ ions in solution.

a) 0.20 M c) 0.40 M e) 0.66 M

b) 0.33 M d) 0.60 M

6. The following reaction:

Pb2+ + 2 I- → PbI2

2 Ce4+ + 2 I- → I2 + 2 Ce3+

HOAc + NH3 → NH4+ + OAc-

are examples of:

a) acid-base reactions.

b) unbalanced reactions.

c) precipitation , acid-base, and redox reactions, respectively.

d) redox, acid-base, and precipitation reactions, respectively.

e) precipitation, redox, and acid-base reactions, respectively.

7. The net ionic equation for the reaction between calcium nitrate and sodium sulfate is:

a) Ca(NO3)2 (aq) + Na2SO4 (aq) → CaSO4 (s) + 2 NaNO3 (aq)

b) Ca2+ (aq) + 2 NO3- + 2 Na+ (aq) + SO42- (aq) → CaSO4 (s) + 2 Na+ (aq) + 2 NO3- (aq)

c) Na+ (aq) + NO3- (aq) (aq) → NaNO3 (s)

d) Ca2+ (aq) + SO42- (aq) → CaSO4 (s)

8. Which of the following salts is insoluble in water?

a) Na2S c) Pb(NO3)2 e) all of these are soluble in water

b) K3PO4 d) Ca(NO3)2

9. Which of the following ions is most likely to form an insoluble sulfate?

a) K+ b) Li+ c) Pb2+

10. In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid, the products are:

a) NaSO4 + H2O c) 2 NaSO4 + H2O e) Na2SO4 + 2 H2O

b) NaSO3 + 2 H2O d) Na2S + 2 H2O

11. What volume (mL) of 0.500 M Cr2(SO4)3 solution is needed to react completely with 300. mL of 0.400 M BaCl2?

a) 60.0 mL c) 85.0 mL e) none of these

b) 80.0 mL d) 160. mL

12. 50.0 mL of 0.10 M silver nitrate is added to 50.0 mL of 0.20 M calcium chloride. A white precipitate forms. After the reaction is complete, calculate the concentration of Cl- ions remaining in solution.

a) 0.20 M c) 0.10 M e) 0.025 M

b) 0.15 M d) 0.050 M

13. A 0.307 g sample of an unknown triprotic acid is titrated to the equivalence point using 35.2 mL of 0.106 M NaOH. Calculate the molar mass of the acid.

H3A + 3 NaOH → Na3A + 3 H2O

a) 247 g/mol c) 165 g/mol e) 82.7 g/mol

b) 171 g/mol d) 151 g/mol

14. Which of the following reactions does not involve oxidation-reduction?

a) CH4 + 3O2 → 2 H2O + CO2

b) Zn + 2 HCl → ZnCl2 + H2

c) 2 Na + 2 H2O → 2 NaOH + H2

d) MnO2 + 4 HCl → Cl2 + 2 H2O + MnCl4

e) all are oxidation-reduction reactions

15. In the following oxidation-reduction reactions, what element is oxidized and what element is reduced?

3 CoSO4 + 5 KI + KIO3 + 3 H2O → 3 Co(OH)2 + 3 K2SO4 + 3 I2

a) Co2+ is oxidized and the I in IO3- is reduced.

b) I- is oxidized and the I in IO3- is reduced.

c) I in IO3- is oxidized and H2O is reduced.

d) I- is oxidized and Co2+ is reduced.

e) none of these is correct.

16. When the equation Cl2 → Cl- + ClO3- (basic solution) is balanced using the smallest whole-number coefficients, the coefficient of OH- is:

a) 1 c) 3 e) 6

b) 2 d) 4

17. The MnO4- is often used to analyze for the Fe2+ content of an aqueous solution via the reaction:

MnO4- + Fe2+ → Fe3+ + Mn2+ (in acidic solution)

A 50.00 mL sample of a solution containing Fe2+ requires 36.43 mL of a 0.025 M KMnO4 solution for complete reaction. The concentration of the Fe2+ in the original solution is:

a) 9.1 X10-2 M c) 4.5 X 10-3 M e) none of these

b) 1.8 X 10-2 M d) 9.1 X 10-4 M

18. Given: 2 MnO4- + 5 H2O2 + 6 H+ → 2 Mn2+ + 8 H2O + 5 O2

What volume of a 0.150 M KMnO4 solution would be needed to titrate 75.0 mL of a 0.150 M H2O2 solution?

a) 15.0 mL c) 45.0 mL e) none of these

b) 30.0 mL d) 75.0 mL

1. b) 5.11 g Chapter: 4 Question: 5

2. d) 0.909 M Chapter: 4 Question: 6

3. a) 400 mL Chapter: 4 Question: 15

4. a) 16 g Chapter: 4 Question: 18

5. c) 0.40 M Chapter: 4 Question: 21

6. e) precipitate, redox, and acid-base reactions, respectively

Chapter: 4 Question: 23

7. d) Ca2+ (aq) + SO42- (aq) → CaSO4 (s) Chapter: 4 Question: 26

8. e) all of these are soluble in water Chapter: 4 Question: 29

9. c) Pb2+ Chapter: 4 Question: 33

10. e) Na2SO4 + 2 H2O Chapter: 4 Question: 37

11. b) 80.0 mL Chapter: 4 Question: 41

12. b) 0.15 M Chapter: 4 Question: 45

13. a) 247 g/mol Chapter: 4 Question: 55

14. e) all are oxidation-reduction reactions Chapter: 4 Question: 61

15. b) I- is oxidized and I in IO3- is reduced Chapter: 4 Question: 66

16. e) 6 Chapter: 4 Question: 77

17. a) 9.1 X 10-2 M Chapter: 4 Question: 81

18. b) 30.0 mL Chapter: 4 Question: 88

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