AP Chem Chapter 4 Pre test

30. The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species? a. 2Br-(aq) b. PO43-(aq) c. 2Ca3(PO4)2(s) d. 6NaBr(aq) e. 3Ca2+(aq)

E. 3Ca 2+(aq)

7. When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? a. hydrogen ion b. acetate ion c. sodium ion d. hydroxide ion e. water

A. Hydrogen ion

6. Select the spectator ions for the following reaction, Pb(NO3)2 + 2 KCl → PbCl2 + 2 KNO3 a. K+(aq), NO3-(aq) b. Pb2+(aq), NO3-(aq) c. K+(aq), Cl-(aq) d. Pb2+(aq), Cl -(aq), K+(aq), NO3-(aq) e. Pb2+(aq), Cl -(aq)

A. K+(aq), NO3-(aq)

23. You have separate solutions of HCl and H2SO4 with the same concentrations in terms of molarity. You wish to neutralize a solution of NaOH. Which acid solution would require more volume (in mL) to neutralize the base? a. The HCl solution. b. The H2SO4 solution. c. You need to know the acid concentrations to answer this question. d. You need to know the volume and concentration of the NaOH solution to answer this question. e. C and D

A. The HCl solution.

10. You have exposed electrodes of a light bulb in a solution of H2SO4 such that the light bulb is on. You add a dilute solution and the bulb grows dim. Which of the following could be in the solution? a. Ba(OH)2 b. NaNO3 c. K2SO4 d. Cu(NO3)2 e. none of these

A.Ba(OH)2

21. In which of the following does nitrogen have the highest oxidation state? a. HNO3 b. NO2 c. N2O d. NH4Cl e. NaNO2

A.HNO3

12. All of the following are weak acids except a. HCNO b. HCl c. HF d. HNO2 e. HCN

B. HCl

4. A solid acid HX is mixed with water. Two possible solutions can be obtained. Which of the following is true? a. In case I, HX is acting like a weak acid, and in case II, HX is acting like a strong acid. b. In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak acid. c. In both cases, HX is acting like a strong acid. d. In both cases, HX is acting like a weak acid. e. HX is not soluble in water.

B. In case I, HX is acting like a strong acid, and in case II, HX is acting like a weak acid.

34. In which of the following does nitrogen have an oxidation state of +4? a. HNO3 b. NO2 c. N2O d. NH4Cl e. NaNO2

B. NO2

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate. 17. The balanced molecular equation contains which one of the following terms? a. AgCl (s) b. 2AgCl (s) c. 2Ba(NO3)2 (aq) d. BaNO3 (aq) e. 3AgCl (aq)

B.2AgCl(s)

19. Identify the precipitate(s) formed (if any) in the following reaction in aqueous solution, Fe(NO3)2 + (NH4)2CO3 → a. Fe2(CO3)3 b. FeCO3(s) c. (NH4)2CO3(s) d. NH4NO3(s) e. No precipitate will be observed

B.FeCO3(s)

14. Which of the following is paired incorrectly? a. H2SO4 - strong acid b. HNO3 - weak acid c. Ba(OH)2 - strong base d. HCl - strong acid e. NH3 - weak base

B.HNO3-weak acid

9. Which of the following compounds is soluble in water? a. Ni(OH)2 b. K3PO4 c. BaSO4 d. CoCO3 e. PbCl2

B.K3PO4

13. Which of the following ions is most likely to form an insoluble chloride? a. K+ b. Li+ c. Ag+ d. S2- e. Cl-

C. Ag+

22. Aqueous solutions of sodium sulfide and copper(II) chloride are mixed together. Which statement is correct? a. Both NaCl and CuS precipitate from solution. b. No reaction will occur. c. CuS will precipitate from solution. d. NaCl will precipitate from solution. e. A gas is released.

C. CuS will precipitate from solution.

15. Which of the following is a strong acid? a. HF b. KOH c. HNO3 d. HCN e. HBrO

C. HNO3

8. When solutions of carbonic acid and magnesium hydroxide react, which of the following are NOT present in the net ionic equation? I. Hydrogen ion II. carbonate ion III. magnesium ion IV. hydroxide ion a. I and II b. I, II, and III c. I and IV d. I and III e. II and III

C. I and IV

28. In writing the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of KOH and Mg(NO3)2 are mixed, which of the following would not be written as ionic species? a. KOH b. Mg(NO3)2 c. Mg(OH)2 d. KNO3 e. All of the above would be written as ionic species.

C. Mg(OH)2

3. In which of the following does nitrogen have the lowest oxidation state? a. HNO3 b. NO2 c. N2O d. NH4Cl e. NaNO2

C. N2O

29. Which of the following is not a strong base? a. Ca(OH)2 b. KOH c. NH3 d. LiOH e. Sr(OH)2

C. NH3

5. Which of the following ions forms the fewest insoluble salts? a. Al3+ b. Cl- c. NH4+ d. OH- e. Mg2+

C. NH4+

11. Which of the following ions forms the fewest insoluble salts? a. Al3+ b. Cl- c. NO3- d. OH- e. Mg2+

C. NO3-

31. You have two solutions of sodium chloride. One is a 2.00 M solution, the other is a 4.00 M solution. You have much more of the 4.00 M solution and you add the solutions together. Which of the following could be the concentration of the final solution? a. 2.20 M b. 3.00 M c. 3.20 M d. 6.00 M e. 6.60 M

C.3.20M

18. The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species? a. 3Al3+(aq) b. OH-(aq) c. 3OH-(aq) d. 2Al3+(aq) e. 2Al(OH)3(s)

C.3OH-(aq)

24. You mix 285.0 mL of 1.20 M lead(II) nitrate with 300.0 mL of 1.60 M potassium iodide. The lead(II) iodide is insoluble. Which of the following is false? a. The final concentration of Pb2+ ions is 0.174 M. b. You form 111 g of lead(II) iodide. c. The final concentration of K+ is 0.821 M. d. The final concentration of NO3- is 0.821 M. e. All are true.

D. The final concentration of NO3- is 0.821 M.

16. You have equal masses of different solutes dissolved in equal volumes of solution. Which of the solutes would make the solution having the highest molar concentration? a. NaOH b. KCl c. KOH d. LiOH e. all the same

D.LiOH

32. In which of the following does iodine have the lowest oxidation state? a. LiIO3 b. IO2 c. I2O d. NH4I e. I2

D.NH4I

2. Which of the following statements is(are) true? Oxidation and reduction a. cannot occur independently of each other b. accompany all chemical changes c. describe the loss and gain of electron(s), respectively d. result in a change in the oxidation states of the species involved e. A, C, and D

E. A, C, and D

25. Which of the following reactions does not involve oxidation-reduction? a. CH4 + 3O2 → 2H2O + CO2 b. Zn + 2HCl → ZnCl2 + H2 c. 2Na + 2H2O → 2NaOH + H2 d. MnO2 + 4HCl → Cl2 + 2H2O + MnCl2 e. All are oxidation-reduction reactions.

E. All are oxidation-reduction reactions.

Which of the following salts is insoluble in water? A. Na2S b. K2CO3 c. Pb(NO3)2 d. CaCl2 e. All of these are soluble in water.

E. All of these are soluble in water.

27. Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed? a. Al3+, S2- b. Pb2+, Cl- c. Ba2+, PO43- d. Pb2+, OH- e. Mg2+, SO42-

E. Mg2+, SO4 2-

20. Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct? a. Both KNO3 and NH4SO4 precipitate from solution. b. A gas is released. c. NH4SO4 will precipitate from solution. d. KNO3 will precipitate from solution. e. No reaction will occur.

E. No reaction will occur.

35. When solutions of barium chloride and ammonium sulfate react, which of the following is a spectator ion? a. barium ion b. chloride ion c. ammonium ion d. sulfate ion e. two of these

E. Two of these

26. Complete the following reaction in aqueous solution and select the spectator ions, Fe(NO3)2 + (NH4)2CO3→ a. Fe2+(aq), NO3-(aq) b. NH4+(aq), NO3-(aq) c. NH4+(aq), CO32-(aq) d. Fe2+(aq), NH4+(aq), NO3-(aq), CO32-(aq) e. Fe2+(aq), CO32-(aq)

b. NH4+(aq), NO3-(aq)

33. Which of the following statements is not true? a. When a metal reacts with a nonmetal, an ionic compound is formed. b. A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction. c. Two nonmetals can undergo an oxidation-reduction reaction. d. When two nonmetals react, the compound formed is ionic. e. A metal-nonmetal reaction involves electron transfer.

d. When two nonmetals react, the compound formed is ionic.