34.62 ml of 0.1510 m

Writing Intensive Course

Chapter 4 Problems

1. Which of these compounds is a strong electrolyte?

A. H2O

B. O2

C. H2SO4

D. C6H12O6 (glucose)

E. CH3COOH (acetic acid)

2. Which of these compounds is a nonelectrolyte?

A. NaF

B. HNO3

C. CH3COOH (acetic acid)

D. NaOH

E. C6H12O6 (glucose)

3. Based on the solubility rules, which one of these compounds should be insoluble in water?

A. NaCl

B. MgBr2

C. FeCl2

D. AgBr

E. ZnCl2

4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?

A. KNO3 will precipitate; Pb2+ and I- are spectator ions.

B. No precipitate will form.

C. Pb(NO3)2 will precipitate; K+ and I- are spectator ions.

D. PbI2 will precipitate; K+ and NO3- are spectator ions.

E. Pb2+ and I- are spectator ions, and PbI2 will precipitate.

5. Give the oxidation # for the following atoms:

a. N in NaNO3 _________

b. Mn in KMnO4 _________

c. Cl in ClO3- _________

6. Which of these equations does not represent an oxidation-reduction reaction?

A. 3Al + 6HCl ( 3H2 + AlCl3

B. 2H2O ( 2H2 + O2

C. 2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3

D. 2NaI + Br2 ( 2NaBr + I2

E. Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu

7. What element is oxidized in the chemical reaction NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?

A. Ni

B. Cd

C. O

D. H

E. This is not a redox reaction.

8. Which of these chemical equations describes a precipitation reaction?

A. 2H2(g) + O2(g) ( 2H2O(l)

B. CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)

C. 2KNO3(s) ( 2KNO2(s) + O2(g)

D. 2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)

E. 2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)

9. The common constituent in all acid solutions is

A. H2.

B. H+.

C. OH-.

D. H2SO4.

E. Cl-.

10. Which of these chemical equations describes an acid-base neutralization reaction?

A. 2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)

B. SO2(g) + H2O(l) ( H2SO3(g)

C. LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)

D. 2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)

E. CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)

11. Which of these chemical equations describes a combustion reaction?

A. 2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)

B. LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)

C. N2(g) + 3H2(g) ( 2NH3(g)

D. 2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)

E. 2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)

12. What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?

13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?

14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?

15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?

16. 34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H2SO4 solution. What is the concentration of the original sulfuric acid solution?

17. Which substance is acting as a Brønsted acid in the following reaction? HSO4- + NH4+ ( H2SO4 + NH3

18. Zinc dissolves in hydrochloric acid to yield hydrogen gas: Zn(s) + 2HCl(aq) ( ZnCl2(aq) + H2(g) What mass of hydrogen gas is produced when a 7.35 g chunk of zinc dissolves in 500. mL of 1.200 M HCl? (Solve this the same way you would any stoichiometry problem. First convert both reagents to moles. For the HCl, use the molarity equation).

19. Complete and balance the following molecular equation (including states of matter). Then write the ionic and net ionic equations.

Fe2(SO4)3 + Na2S (