AP Chemistry - Ch4 Homework
Ch4 HW#1 p180+ 11(d-g),13,15(a,b),17(a,b)
11. Show how each of the following strong electrolytes “ breaks up” into its
component ions dissolving in water.
d. (NH4)2SO4
e. HI
f. FeSO4
g. KMnO4
h. HClO4
13. Calciun chloride is a strong electrolyte and is used to “salt” streets in the winter to melt ice and snow.
Write a reaction to show how this substance breaks apart when it dissolves in water.
15.Calculate the molarity of each of these solutions.
a. A 5.623g sample of NaHCO3 is dissolved in enough water to make 250 ml of solution.
b. A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make 500 ml of solution.
17. Calculate the concentration of all ions present in each of the following solutions of strong electrolyte
a. 0.15 M CaCl2
b. 0.26 M Al(NO3)3
Ch4 HW#2 p181 21,23(a,b),25
21. What volume of a 0.100 M solution of NaHCO3 contains 0.350 g of NaHCO3?
23. Describe how you would prepare 2.00 L of each of the following solutions.
a. 0.250M NaOH from solid NaOH
b. 0.250M NaOH from 1.00M NaOH stock solution
25. A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 200.0 mL of stock solution.
A 10.0 mL sample of this stock solution is added to 50.0 mL of water. Calculate the concentration of ammonium ions
and sulfate ions in the final solution.
Ch4 HW#3 p181+ 29,31,33,35(a,b)
29. When the following solutions are mixed together, what precipitation (if any) will form?
a. BaCl2(aq) + NaSO 4(aq)
b. Pb(NO3)2(aq) + KCl(aq)
c. AgNO3(aq) + Na3PO4(aq)
d. NaOH(aq) + Fe(NO3)3(aq)
31. For the reactions in Exercise 29, write the balanced molecular equation, complete ionic equation,
and net ionic equation. If no precipitate forms, write “No reaction.”
33. Write net ionic equations for each of the following.
a. AgNO3(aq) + KI(aq)
b. CuSO4(aq) + Na2S(aq)
c. CoCl2(s) + NaOH(aq)
d. NiCI2(aq) + KNO3(aq)
35. Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.
a. Ammonium sulfate and barium nitrate
b. Lead(II) nitrate and sodium chloride
Ch4 HW#4 p182 39,41,43
39. What mass of NaCl is required to precipitate all the silver ions from 50.0 mL of a 0.0500 M solution of AgNO3?
41. What mass of solid aluminum hydroxide is produced when 50.0 mL
of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 mL M KOH?
43. A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed
with 100.0 mL of 0.200 M aqueous magnesium nitrate.
a. Write a balanced chemical equation for any reaction that occurs.
b. What precipitate forms?
c. What mass of precipitate is produced?
d. Calculate the concentration of each ion remaining in solution after precipitation is complete.
Ch4 HW#5 p182 44
44. How many grams of silver chloride can be prepared by the reaction of 100.0mL of 0.20M silver nitrate
with 100.0mL of 0.15M calcium chloride?
Calculate the concentration of each ion remaining in solution after precipitation is complete.
Ch4 HW#6 p182 45(a,b),47(a,b),49(a,b) + Lab4.2 Pre-lab questions
45. Write the balanced molecular, complete ionic, and net ionic equations for each of the following acid-base reactions.
a. HClO4(aq) + Mg(OH)2(s) →
b. HCN(aq) + NaOH(aq) →
47. Write the balanced molecular, complete ionic, and net ionic equations for the reactions that occur when
the following are mixed.
a. potassium hydroxide (aqueous) and nitric acid
b. barium hydroxide (aqueous) and hydrochloric acid
49. What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH?
a. 0.100 M HCl
b. 0.150 M HNO3
Pre-lab questions: The following data was obtained from a regular chemistry lab group conducting this lab:
Trial 1
NaOH
Initial Volume Final Volume
Volume Used
Molarity
0.100M
1mL
12mL
HCl
Initial Volume Final Volume
Volume Used
Molarity
2mL
9mL
1. Fill in the rest of the data table.
2. Show your calculation for the Molarity of the HCl solution. Leave the answer on the calculator screen.
3. Knowing my regular chem classes, this trial may have lacked accuracy, but it definitely lacked precision.
Please list the obvious non-precise measurements.
4. Look at your calculator answer. Round the answer to the correct number of significant digits.
If you look at the first 3 digits on your calculator screen, how different do your 2 answers look?
5. If the actual molarity of HCl was 0.150M, please find the % error for the answer with the correct sig digs.
6. Can you see how precise measuring can be as important as accurate measuring?
Ch4 HW#7 Mid Chapter Review p180+ 16c,18c,24b,54
16c. A 0.4508-g sample of iron is dissolved in a small amount of concentrated nitric acid forming Fe3+ ions in solution
and is diluted to a total volume of 500.0ml. Calculate the molarity of Fe3+.
18c. Calculate the concentration of all ions present in 5.00g of NH4Cl in 500.0mL of solution.
24b. How would you prepare 1.00 L of 0.500M HCl from “concentrated” (12M) reagent?
54. What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?
Ch4 HW#8 p182+ 57,59,61(a,b) ALL of these are test worthy!
57. Assign oxidation states for all atoms in each of the following compounds.
a. KMnO4
b. NiO2
c. K4Fe(CN)6 (Fe only)
d. (NH4)2HPO4
e. P4O6
f. Fe3O4
g. XeOF4
h. SF4
i. CO
j. Na2C2O4
59. Assign the oxidation for chlorine in each of the following anion:
OClClO2- CLO3- CLO461(a,b). Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent,
the reducing agent, the substance being oxidized, and the substance being reduced.
a. CH4(g) + 2O2(g)
CO2(g) + 2H2O(g)
b. Zn(s) + 2HCI(aq)
ZnCI2(aq) + H2(g)
Ch4 HW#9 p183 63(a,b), 65(a) ALL of these are test worthy!
63. Balance the following oxidation-reduction reactions that occur in acidic solutions.
a. Zn(s) + HCl(aq)
Zn2+(aq) + H2(g)
b. I-(aq) + ClO-(aq)
I3-(aq) + Cl-(aq)
65. Balance the following oxidation-reductions reactions that occur in acidic solutions.
a. Al(s) + MnO4-(aq)
MnO2(s) + Al(OH)4-(aq)
Ch4 HW#10 p183 64(a,b),66(a)
64. Balance the following oxidation-reduction reactions that occur in acid solution using the half-reactions method.
a. Cu(s) + NO3-(aq)
Cu2+(aq) + NO(aq)
b. Cr2O72-(aq) + Cl-(aq)
Cr3+(aq) + Cl2(g)
66. Balance the following oxidation-reduction reactions that occur in acidic solution.
a. Cr(s) + CrO42(aq)
Cr(OH)3(s)
Ch4 Rev#1 p180+ 12c,16b,18d, 22,24e,36(a,b) Ch4 Rev#2 p180+ 42,53,62a,67
12c. Show how Ca(OH)2 “breaks up” into its component ions dissolving in water.
16b. An 853.5-mg sample of KIO3 is dissolving in enough water to make 250.0 mL of solution. Calculate the molarity.
18d. Calculate the concentration of all ions present of 1.00 g K3PO4 in 250.0 mL of solution.
22. How many grams of NaOH are contained in 250.0 mL of a 0.400 M sodium hydroxide solution.
24e. How would you prepare 1.00 L of a 0.50 solution of sodium carbonate from the pure solid.
36. Write net ionic equations for the reaction, if any, when aqueous solutions of the following are mixed.
a) Cobalt(III) chloride and sodium hydroxide.
b) Silver nitrate and ammonium carbonate.
42. What mass of barium sulfate is produced when 100.0 mL of a 0.100 M solution of barium chloride
is mixed with 100.0 mL of a 0.100 M solution of iron(III) sulfate?
53. A 25.00 mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide
for complete neutralization.
What is the concentration of the original hydrochloric acid solution?
62a. Specify if Cu(s) + 2Ag+(aq)  2Ag(s) + Cu+2(aq) is an oxidation-reduction reaction,
and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced.
67. Chlorine gas was first prepared in 1774 by C.W. Scheele by oxidizing sodium chlorine with manganese(IV) oxide.
The reaction is: NaCl(aq) + H2SO4(aq) + MnO2(s)  Na2SO4(aq) + MnCl2(aq) + H2O(l) + Cl2(g)