AP Chem: Chapter 4 Practice Multiple Choice Questions

[Pages:6]AP Chem: Chapter 4 Practice Multiple Choice Questions

Multiple Choice Identify the choice that best completes the statement or answers the question.

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1. What mass of silver nitrate, AgNO3, is required to prepare 800. g of 3.50% solution of AgNO3? a. 24.6 g b. 26.7 g c. 27.0 g d. 25.5 g e. 28.0 g

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2. What mass of water is contained in 160. grams of 22.0% KCl solution? a. 125 g b. 86.8 g c. 35.2 g d. 130 g e. 112 g

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3. The density of a 7.50% solution of ammonium sulfate, (NH4)2SO4, is 1.04 g/mL. What mass of (NH4)2SO4 would be required to prepare 750. mL of this solution? a. 45.8 g b. 54.0 g c. 58.5 g d. 62.4 g e. 65.7 g

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4. What volume of 40.0% NaNO3 solution contains 0.15 mole of NaNO3? Density = 1.32 g/mL. a. 42.0 mL b. 3.86 mL c. 9.60 mL d. 24.1 mL e. 38.2 mL

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5. What is the molarity of 175 mL of solution containing 2.18 grams of Na2SO4?10H2O? a. 3.77 10-3 M b. 6.44 10-1 M c. 8.78 10-3 M d. 1.18 10-3 M e. 3.87 10-2 M

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6. What mass of Na2SO4 is required to prepare 400. mL of 1.50 M Na2SO4 solution? a. 213 g b. 56.8 g c. 71.4 g d. 85.2 g e. 8.52 104 g

____ 7. Calculate the molarity of the resulting solution if 25.0 mL of 2.40 M HCl solution is diluted to 300. mL. a. 0.200 M

b. 29.0 M c. 2.00 M d. 0.400 M e. 0.0400 M

____ 8. Silver nitrate, AgNO3, reacts with sodium chloride as indicated by the following equation. What mass of NaCl would be required to react with 200. mL of 0.200 M AgNO3 solution?

AgNO3 + NaCl AgCl + NaNO3

a. 0.117 g b. 1.17 g c. 2.34 g d. 4.68 g e. 3.06 g

____ 9. What volume of 0.130 M HCl solution will just react with 0.424 gram of Ba(OH)2?

2HCl + Ba(OH)2 BaCl2 + 2H2O

a. 38.1 mL b. 32.6 mL c. 24.1 mL d. 18.6 mL e. 96.7 mL

____ 10. What is the total ionic equation for the following formula unit equation?

HF(aq) + KOH(aq) KF(aq) + H2O(l)

a. [H+(aq)+F-(aq)] + [K+(aq)+OH-(aq)] [K+(aq)+F-(aq)] + [2H+(l)+O2-(l)] b. [H+(aq)+F-(aq)] + [K+(aq)+OH-(aq)] [K+(aq)+F-(aq)] + H2O(aq) c. HF(aq) + [K+(aq)+OH-(aq)] [K+(aq)+F-(aq)] + H2O(l) d. HF(aq) + [K+(aq)+OH-(aq)] [K+(aq)+F-(aq)] + [2H+(aq)+OH-(aq)] e. HF(aq) + OH-(aq) F-(aq) + H2O(l)

____ 11. What is the oxidizing agent in the following reaction?

8H+(aq) + 3C2H5OH(aq) + Cr2O72-(aq) 2Cr3+(aq) + 3C2H4O(aq) + 7H2O(l)

a. H+ b. Cr2O72c. Cr3+ d. C2H5OH e. H2O

____ 12. Which response includes all the following that are oxidation-reduction reactions, and no others?

I. BaSO3(s) BaO(s) + SO2(g) II. 2K(s) + Br2(l) 2KBr(s) III. H2CO3(aq) + Ca(OH)2(aq) CaCO3(s) + 2H2O(l)

IV. SnS2(s) + 6HCl(aq) H2SnCl6(s) + 2H2S(aq) V. 3Cl2(g) + 6KOH(aq) 5KCl(aq) + KClO3(aq) + 3H2O(l)

a. II, III, and IV b. I and III c. II and V d. I and IV e. another one or another combination

____ 13. What is the reducing agent in the following reaction?

Cu(s) + 4H+(aq) + SO42-(aq) Cu2+(aq) + 2H2O(l) + SO2(g)

a. Cu b. H+ c. SO42d. Cu2+ e. SO2

____ 14. Which of the following reactions is a combination reaction? a. AgNO3(aq) + HCl(aq) AgCl(s) + HNO3(aq) b. Na2O(s) + CO2(g) Na2CO3(s) c. C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) d. 2H2O(l) 2H2(g) + O2(g) e. KOH(aq) + HCl(aq) KCl(aq) + H2O(l)

____ 15. Write the balanced total ionic equation for the complete reaction of phosphoric acid and calcium hydroxide. What is the coefficient preceding water in this equation? a. 6 b. 8 c. 12 d. 4 e. 5

____ 16. Write the balanced net ionic equation for the complete neutralization of chromium (III) hydroxide with sulfuric acid. Use H+ rather than H3O+. What is the sum of the coefficients? (Do not forget coefficients of one.) a. 11 b. 8 c. 16 d. 18 e. 22

____ 17. Will a precipitate form when 0.1 M aqueous solutions of HBr and Pb(CH3COO)2 are mixed? If a precipitate

does form, identify the precipitate and give the net ionic equation for the reaction.

a. PbBr2 precipitates.

2[H+(aq)+Br -(aq)] + [Pb2+(aq)+2CH3COO-

b. CH3COOH precipitates. c. PbBr2 precipitates.

(aq)] PbBr2(s) + 2CH3COOH(aq) H+(aq) + CH3COO-(aq) CH3COOH(s) Pb2+(aq) + 2Br -(aq) PbBr2(s)

d. PbBr2 precipitates.

Pb(CH3COO)2(aq) + 2Br -(aq) + 2CH3COO-(aq)

PbBr2(s)

e. No precipitate forms.

____ 18. Will a precipitate form when 0.1 M aqueous solutions of Ba(NO3)2 and H2CO3 are mixed? If a precipitate

does form, identify the precipitate and give the net ionic equation for the reaction.

a. No precipitate forms.

b. BaCO3 precipitates.

Ba2+(aq) + CO32-(aq) BaCO3(s)

c. BaCO3 precipitates.

Ba2+(aq) + H2CO3(aq) BaCO3(s) + H2(g)

d. BaCO3 precipitates.

Ba2+(aq) + H2CO3(aq) BaCO3(s) + 2H+(aq)

e. H2(NO3)2 precipitates. 2H+(aq) + 2NO3-(aq) H2(NO3)2(s)

____ 19. The equation, 2H+(aq) + CO32-(aq) aqueous mixture of a. CaCO3 and HCl. b. Na2CO3 and HCl. c. H2CO3 and NaOH. d. BaCO3 and H2SO4. e. (COOH)2 and KOH.

H2O(l) + CO2(g), is the net ionic equation for the reaction of an

____ 20. Which of the following is not a metathesis reaction?

a. CH4(g) + 2O2(g) CO2(g) + 2H2O(l) b. FeS(s) + 2HCl(aq) FeCl2(aq) + H2S(g) c. CaCl2(aq) + K2CO3(aq) CaCO3(s) + 2KCl(aq) d. 2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2H2O(l) e. AgNO3(aq) + NaBr(aq) AgBr(s) + NaNO3(aq)

____ 21. Which of the following reactions is (are) metathesis reactions?

I. 2NaCl(aq) + Hg2(NO3)2(aq)

a. only I b. only II c. only III d. only I and II e. only I and III

____ 22. Classify the following reaction by giving all of these reaction type(s) that apply.

I. redox II. combination III. decomposition IV. displacement V. metathesis

2PbO(s) + O2(g) 2PbO2(s)

a. I and V b. only II c. I and II d. only III e. only V

____ 23. Classify the following reaction by giving all of these reaction type(s) that apply.

I. redox II. combination III. decomposition IV. displacement V. metathesis

CaCO3(s)

CaO(s) + CO2(g)

a. only I b. only II c. only III d. only IV e. I and V

____ 24. Classify the following reaction by giving all of these reaction type(s) that apply.

I. redox II. combination III. decomposition IV. displacement V. metathesis

Ba(OH)2(aq) + Na2CO3(aq) BaCO3(s) + 2NaOH(aq)

a. only I b. only II c. only V d. only IV e. II and III

____ 25. Classify the following reaction by giving all of these reaction type(s) that apply.

I. redox II. combination III. decomposition IV. displacement V. metathesis

P4(s) + 10Cl2(g) 4PCl5(g)

a. I and V b. only II c. only III d. I and II e. only V

AP Chem: Chapter 4 Practice Multiple Choice Questions Answer Section

MULTIPLE CHOICE

1. ANS: E 2. ANS: A 3. ANS: C 4. ANS: D 5. ANS: E 6. ANS: D 7. ANS: A 8. ANS: C 9. ANS: A 10. ANS: C 11. ANS: B 12. ANS: C 13. ANS: A 14. ANS: B 15. ANS: A 16. ANS: B 17. ANS: A 18. ANS: D 19. ANS: B 20. ANS: A 21. ANS: D 22. ANS: C 23. ANS: C 24. ANS: C 25. ANS: D

PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1 PTS: 1

TOP: Concentrations of Solutions TOP: Concentrations of Solutions TOP: Concentrations of Solutions TOP: Concentrations of Solutions TOP: Concentrations of Solutions TOP: Concentrations of Solutions TOP: Dilution of Solutions TOP: Using Solutions in Chemical Reactions TOP: Using Solutions in Chemical Reactions TOP: Reactions in Aqueous Solutions TOP: Oxidation-Reduction Reactions-An Introduction TOP: Oxidation-Reduction Reactions-An Introduction TOP: Oxidation-Reduction Reactions-An Introduction TOP: Combination Reactions TOP: Metathesis (Acid-Base) Reactions TOP: Metathesis (Acid-Base) Reactions TOP: Metathesis (Precipitation) Reactions TOP: Metathesis (Precipitation) Reactions TOP: Metathesis (Gas-Formation) Reactions TOP: Metathesis (Gas-Formation) Reactions TOP: Summary of Reaction Types TOP: Summary of Reaction Types TOP: Summary of Reaction Types TOP: Summary of Reaction Types TOP: Summary of Reaction Types

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