CHEM 1115 Unit 5 Practice Problems

 

 

1.      Complete and balance the following reactions.  Include the physical state of each of the products.

 

      a)       BaCl2(aq)  +     Na2SO4(aq)  ®

 

      b)       AlCl3(aq)  +       AgNO3(aq)  ®

 

 

2.      Write the complete ionic equation and the net ionic equation for the following:

 

a)  Fe(NO3)3(aq) + 3KOH(aq) ® Fe(OH)3(s) + 3KNO3(aq)

 

b)  3Fe(C2H3O2)2(aq) + 2Na3PO4(aq) ® Fe3(PO4)2(s) + 6NaC2H3O2 (aq)

 

 

 

3.      Complete and balance the following acid-base neutralization reactions.  Write the complete ionic equation and the net ionic equation for each reaction.

 

      a)  Fe(OH)3(s)  +        HCl(aq) ®

 

      b)  Al(OH)3(s)  +       H2SO4(aq) ®

 

 

4.      Determine the oxidation numbers of all of the elements in the following compounds:

 

a)   Ca(MnO4)2             b)   KHSO3              c)  K2S2O3      d) (NH4)2SO4      e)   O2

 

 

 

5.      Write complete ionic and net ionic equations for the following reactions:

 

      Pb(s) +  Cu(NO3)2 (aq) ®  Pb(NO3)2  (aq) + Cu(s)

 

      Fe(s) +  2HCl(aq) ®  FeCl2 (aq) +  H2(g)

 

 

6.      Each reaction shown in question 5 is a redox reaction.  For each reaction, identify the element oxidized, element reduced, oxidizing agent, and reducing agent.

 

7.      What volume of 1.30 M K2SO4 is needed to provide 0.330 mol K2SO4 for a reaction?

 

8.      What volume of 2.00 M NaClO3 contains 60.0 g of NaClO3?

 

9.      What volume of 2.40 M MgCl2 is needed to provide 0.225 mol of chloride ion to a reaction?

 

10.  What mass of Na2SO4 is needed to make 250.0 mL of 0.850 M Na2SO4?

 

11.  Describe in detail how you would prepare 500.0 mL of 1.00 M NaCl from solid NaCl.

12.  What volume of 12.0 M HCl is needed to prepare 600.0 mL of 1.75 M HCl?

 

13.  Describe in detail how you would prepare 250.0 mL of 2.0 M HCl from 12.0 M HCl.

 

14.  What is the molarity of a solution prepared by dissolving 85.0 g of NaCl in enough water to make 125 mL of solution?

 

15.  How many grams of calcium carbonate can be produced by reacting 50.0 mL of 0.50 M sodium carbonate with an excess of calcium chloride? (Hint:  Write a balanced equation first.)

 

16.  How many mL of 0.15 M calcium chloride is needed to react completely with 37.5 mL of 0.25 M sodium carbonate?  (Hint:  Write a balanced equation first.)

 

17.  How many mL of 0.25 M phosphoric acid are needed to react completely with 25.0 mL of  0.25 M calcium hydroxide? (Hint: Write a balanced equation first.)

 

18.  What is the concentration of an H2SO4 solution if 80.0 mL is neutralized by 36.2 mL of 1.50 M NaOH?

 

                        2NaOH + H2SO4 ® 2H2O + Na2SO4

19.  Draw the Lewis structure for the following substances:  NO2-, carbonate ion, nitrate ion, perchloric acid, CH2O.

 

20.  Identify the electron domain and molecular geometries for each substance in the previous question.

 

21.  Calculate the volume of 22.0 g of a substance that has a density of 1.24 g/mL.

 

22.  Write a balanced equation for the reaction between aqueous solutions of sodium bicarbonate and phosphoric acid.  Identify the acid.  Identify the base.

 

23.  Write the electron configuration for arsenic.  Write its electron configuration using core notation.

 

24.  Which of the following atoms is larger:  Li  or Sn?

 

25.  Which of the following is larger:  Cl or Cl- ?

 

26.  Which one of the following has the larger ionization energy:  Mg or Ba?