CHM 2046C Module 11i-Chapter 15 Name:______
Module 11i: Acids and Bases: A Molecular Look Jesperson Chapter 15 / Possible / ActualA. Idenification of Bronsted-Lowry acids&bases - Section15.1 / 1 / Answer
B. Idenitication of Lewis Acids and Bases – Section 15.4 / 1
C. Writing Ionization Reactions Strong/Weak Arrhenius Acid/Bases Section 4.4 / 1 / Answers
C1. Strengths of Bronsted-Lowry Acids and Bases – Section 15.2 / 1
C2. Periodic Trends in Strengths of Acids – Section 15.3 / 1
D. Determination of pH & pOH from concentrationsProblems Section 16.1 / 2 / Answer
D. pH Sample 2 / Answer
W. Rewriting Equations Ionically Section 4.8 / 5 / Answers
Answer Explained / Answer
R. Balancing REDOX Equation via Ion Electron Method Section 5.2 / 6 / Answers
Module Eleven Total: / 20
Part A: Identification of Bronsted-Lowry Acids and Bases 1 point
Label the acid and the base and their corresponding conjugate B/L pairs for the following reactions:
(1) NH4 + + Cl 1- <=====> NH3 + HCl
(2) CH3OH + Cl1- <======> HCl + CH3O1-
(3) C5H5NH+1 + H2O <======> C5H5N + H3O+1
(4) HSeO4 1- + NH3 <======> NH4 1+ + SeO4 2-
(5) HCO3 1- + OH 1- <======> CO3 2- + H2O
Reference: Jespersen Section 15.1
Look at Example 15.1 page 735; Exam 15.2 page 736
Try Practice 15.1 and 15.2 Page 735; Try 15.3 and 15.4 page 736
Try 15.5 and 15.6 page 737 Review Question 15.1-15.5 Page 758
Try ReviewProblesm 15.49-15.54 Pages 759-760
Answers: http://www.fccj.us/chm2046/SampleTest/46M11abAnswer.htm
CHM 2046C Module 11i Homework Packet
Part B: Identification of Lewis Acids and Bases 1 point
Draw Lewis Symbols and Identify the Lewis Acid and base in the following reactions: (Hint you need to draw the dot structure and Lewis symbols to diagram the reaction, then label the LA and LB)
(1) NH3 + BF3 <======> NH3BF3
(2) CO2 + OH 1- <======> HCO3 1-
(3) SO2 + O 2- <==+======> SO3 2-
(4) NH3 + H 1+ <======> NH4 1+
List four types of substances that are Lewis Acids (Table 15.3 Page 748)
(1)
(2)
(3)
(4)
List one type of substance that is a Lewis Base:
(1)
Reference: Jespersen Section 7.4
Try Practice Exercises 15.17 and 15.18 Page 749
Look at Review Questions 15.25-15.32 Page 759
Try Review Problems 15.61-15.68 Page 760
CHM 2046C Module 11i Homework Packet
Part C: Writing Ionization Reactions Strong/Weak Arrhenius Acid/Bases 1 point
Write the ionization reactions for the following:
(1) Strong Acid: HCl (aq)
(2) Weak Acid: HC2H3O2 (aq)
(3) Strong Base: NaOH (aq)
(4) Weak Base: NH3 (aq)
(5) Weak Acid: H3PO4 (aq) (show all three ionization reactions)
Reference Jespersen Section 4.4
Try Practice 4.5 and 4.6 Page 167
Look at Example 4.3 page169; Try Practice 4.7 and 4.8 Page 169
Look at Example 5.4 Page 171 Try Practice 4.9 and 4.10 Page 171
Answer Review Questions 4.13-4.25 Page 205
Review Problems 4.51-4.60 Page 207
CHM 2046C Module 11i Homework Packet
Part C1 Strengths of Bronsted-Lowry Acids and Bases: 1 Point
1. Which of the following is the strongest acid: HClO4 , HNO2 , or H3O1+ ?
2. Which of the following is the strongest base: NaOH; NH4OH; or OH1- ?
3. On page 739 of the Jespersen text, the following reaction is show explaining the relative strength and weaknesses of Bronstead Acid-Base pairs: Oxide and hydroxide:
O2 - + H2O ----> OH - + OH -
Correct the misprint and label the acid-conjugate base pair and the Base conjugate acid pair.
4. Given that HSO41- is a stronger acid than HPO41- write the chemical reaction if the solution containing both of these ions are mixed together. (Hint one of these must act as an acid and the other as a base)
Reference: Jespersen Section 15.2
Look at Example 15.3 page 740
Try Practice Exercise15.7 and 15.8 page 741
Try Review Questions 15.6-15.13 page 758
Try Review Problems 15.82-15.85 page 761
CHM 2046C Module 11i Homework Packet
Part C2 Periodic Trends in the Strengths Acids and Bases: 1 Point
(1) Circle the stronger acid in the following acid pairs:
HBr or HI H2S of HCl PH3 or NH3
(2) Circle the stronger acid in the following acid pairs:
HClO or HClO2 H2SeO3 or H2SeO4
(3) Circle the stronger acid in the following acid pairs:
HClO4 or HClO3 HIO2 or HClO3
(4) Circle the stronger acid in the following acid pairs:
H3AsO4 or H3PO4 H2CO3 or HNO3
Reference: Jespersen Section 15.3
Look at Tables 15.1 Page 741 and Table 15.2 Page 742
Try Practice Exercise15.9 and 15.10 page 742
Try Practice Exercise15.11 and 15.12 page 744
Try Practice Exercise15.13 and 15.14 page 745
Try Review Questions 15.14-15.15 page 758
Try Review Problems 15.55-15.60 page 760
CHM 2046C Module 11i Homework Packet
Part D: pH Scale Calculations 2 points
What is the pH and pOH of the following solutions:
(1) 0.000675 M HCl
(2) 0.0025 M Ca(OH)2
(3) The pH of a cup of coffee is 4.32, calculate the [H3O+1 ]:
(4) A detergent solution has a pH of 11.45. What is the [OH 1- ]?
Reference: Sections 16.1 and 16.2
Try Practice 16.1 and 16.2 Page 765
Try Practice 16.3, 16.4, and 16.5 Page 767
Try Practice 16.6 and 16.7 Page 768
Answer Review Questions 16.8-16.13 Pages 808-809
Review Problems 16.49-16.62 Page 810
Answers: http://www.fccj.us/chm2046/SampleTest/46M11dAnswer.htm
CHM 2046C Module 11i Homework Packet
Module 11i: Part W1 Rewriting Equations Ionically 1 point
Rewrite the following (unbalanced) equations ionically, balance the molecular equation 1st; cancel spectator ions and then show the balance the net ionic reactions.
Show as ions: soluble salts and strong acids; leave as molecules/formula units insoluble salts, weak acids, covalent molecules. Strong acids are: Perchloric Acid; Hydrochloric Acid; Nitric Acid; Sulfuric Acid; Hydrobromic Acid; Hydroiodic Acid
1. KOH (aq) + HNO3(aq) à KNO3(aq) + HOH(l)
2. CuSO4 (aq) + Na2CO3 (aq) à CuCO3 (s) + Na2SO4 (aq)
3. NaOH (aq) + NH4NO3 (aq) à NaNO3 (aq) + NH3 (g) + HOH (l)
4. BaBr2 (aq) + ZnSO4 (aq) à BaSO4 (s) + ZnBr2 (aq)
5. Cr(OH)2 (s) + HCl (aq) à
Reference: Jespersen Section 4.3
Look at Example 4.2 Page 162
Try Practice 4.3 and 4.4 Page 163
Look at Review Questions 4.11 and 4.12 Page 205
Try Review Problems 4.47-4.50 Page 206
Answers to Above: http://www.fccj.us/chm2045/SampleTest/45m8gAnswer.htm
Module 11i: Part W2 Rewriting Equations Ionically REDOX 4 points
REDOX Equations: Writing Net Ionic Write net unbalanced ionic reactions for 20 of the following:
The following Unbalanced Acid and Basic Media REDOX equations need to be re-written ionically Unbalanced. Rewrite the following Unbalanced chemical equations ionically in total ionic form (without balancing), then cancel spectators for the net ionic equation. Do not forget to place charges on the ions and no charge on the molecules/formula units. This is Step#1 in REDOX balancing so the equations can not be balanced first as shown in the book (and as on the test item M-8G.)
Rewrite as ions electrolytes such as
(a) Soluble salts,
(b) Strong acids, Some strong acids are hydrochloric acid, nitric acid, sulfuric acid, perchloric acid, hydrobromic acid and hydroiodic acid.
(c) Strong bases. Strong bases include KOH and NaOH and any soluble hydroxide. Soluble salts are those ionic hydroxide compounds with (aq) (water solution: therefore soluble).
Reference: CHM 1025C: Corwin: Section 14.11 HeinSection 15.7
CHM 2045C: McMurry: Section 4.3 Jespersen Section 4.3
1. Zn (s) + HNO3 (aq) ---> Zn(NO3)2 (aq) + NH4NO3 (aq) + H2O (l)
2. KMnO4(aq)+K2C2O4(aq)+HCl(aq)--->MnCl2(aq)+CO2(g)+KCl(aq)+H2O(l)
3. K2Cr2O7 (aq) + HCl (aq) ---> CrCl3 (aq) + Cl2 (g) + KCl (aq) + H2O (l)
4. Cu (s) + HNO3 (aq) ---> Cu(NO3)2 (aq) + NO2 (g) + H2O (l)
5. Cu (s) + HNO3 (aq) ---> Cu(NO3)2 (aq) + NO (g) + H2O (l)
6. KI (aq) + HNO3 (aq) ---> NO (g) + I2 (s) + KNO3 (aq) + H2O (l)
7.K2Cr2O7(aq)+C2H5OH(aq)+HCl(aq)---CrCl3(aq)+HC2H3O2(aq)+KCl(aq)+H2O(l)
8. CH2O (l) + H2SO4 (aq) ---> H2S (g) + CO2 (g) + H2O (l)
9. Zn (s) + HNO3(aq) ---> N2 (g) + Zn(NO3)2 (aq) + H2O
10. Zn (s) + HNO3(aq) ---> N2O (g) + Zn(NO3)2 (aq) + H2O (l)
11: KMnO4(aq) + K2C2O4 (aq) + KOH(aq) ---> MnO2(s) + K2CO3 (aq) + H2O(l)
12: KMnO4 (aq) + KIO (aq) + H2O(l) ---> MnO2(s) + KIO4(aq) + KOH(aq)
13: K2C4H4O6 (aq) + KClO3(aq) + KOH(aq) ---> K2CO3(aq) + KCl (aq) + H2O(l)
14: KMnO4(aq) + KCN(aq) + H2O (l) ---> MnO2(s) + KCNO (aq) + KOH(aq)
15: Na2S(aq) + I2(s) + NaOH (aq) ---> Na2SO4 (aq) + NaI(aq) + H2O (l)
16: Cr(OH)3(s) + Cl2(g) + NaOH (aq) ---> NaCl (aq) + Na2CrO4(aq) + H2O (l)
17. Fe(OH)2(s) + O2(g) + H2O(l) ---> Fe(OH)3(s)
18. K3Fe(CN)6(aq)+Cr2O3(s)+ KOH (aq ---> K4Fe(CN)6 (aq)+ K2CrO4 (aq) + H2O(l)
19: NaBH4(aq) + NaClO3(aq ---> NaH2BO3(aq) + NaCl(aq) + H2O (l)
20. NaAlH4(aq)+ H2CO3(aq)+ NaCl(aq)+H2O(l)---> AlCl3(aq)+ CH3OH(l)+ NaOH(aq)
Video:
http://www.brightstorm.com/science/chemistry/chemical-reactions/net-ionic-equation/
Some Answers More Answers NonRedox Answers
Module 11i Part R: Redox Equations 6 points
Your M-11i Exam will have two REDOX equations written in net ionic form. The worked samples are online under the grading outline. You must show your work and you must have correct balanced half equations. You must use the Ion electron Method
Acid Media: (1 Point)
1. C2O4 2- (aq) + MnO4 1- (aq) + H 1+ (aq) → Mn 2+ (aq) + CO2 (g) + HOH (l)
half equation:
half equation:
Final Answer:
C2O4 2- (aq) + MnO4 1- (aq) + H 1+ (aq) → Mn 2+ (aq) + CO2 (g) + HOH (l)
Reference: Section 5.2 Ion-Electron Method
Look at Example 5.5 page 223 Try Practice 5.7 and 5.8 Page 224
Online REDOX Study Guide: http://www.fscj.me/REDOX/REDOXstudy.html
Look at Review Questions 5.6-5.10
Review Problems: 5.43-5.48 Pages 243-244
Some Answers More Answers
Basic Media (1 point)
2. Bi2O3 (s) + OH 1- (aq) + OCl 1- (aq) → BiO3 1- (aq) + Cl 1- (aq) + HOH (l)
half equation:
half equation:
Final Answer:
Bi2O3 (s) + OH 1- (aq) + OCl 1- (aq) → BiO3 1- (aq) + Cl 1- (aq) + HOH (l)
Step by Step Solutions to the two equations above:
http://www.fccj.us/chm2045/SampleTest/45M8hAnswer.htm
For additional Acid Media REDOX Homework-Ion Electron: (.25 points each)
(3) Zn + NO3 1- + H 1+ à Zn 2+ + NH4 1+ + H2O
half equation:
half equation:
Final Answer:
Zn + NO3 1- + H 1+ à Zn 2+ + NH4 1+ + H2O
------
(4) Cr2O7 2- + C2H5OH + H 1+ à Cr 3+ + HC2H3O 2 + H2O
half equation:
half equation:
Final Answer:
Cr2O7 2- + C2H5OH + H 1+ à Cr 3+ + HC2H3O 2 + H2O
(5) FeS + NO3 1- + H 1+ à NO + Fe 2+ + SO4 2- + H2O
half equation:
half equation:
Final Answer:
FeS + NO3 1- + H 1+ à NO + Fe 2+ + SO4 2- + H2O
------
(6) H2O2 + MnO4 1- + H 1+ à Mn 2+ + O2 + H2O
half equation:
half equation:
Final Answer:
H2O2 + MnO4 1- + H 1+ à Mn 2+ + O2 + H2O
(7) C12H22O11 + H2SO4 + K2Cr2O7 à CO2 + Cr2(SO4)3 + K2SO4 + H2O (0.50 points)
Net Ionic:
half equation:
half equation:
Final Answer:
C12H22O11 + H2SO4 + K2Cr2O7 à CO2 + Cr2(SO4)3 + K2SO4 + H2O
------
(8) As2S5 + KNO3(aq) + HNO3(aq) à NO2 + H3AsO4(aq) + KHSO4(aq) + H2O
(9) Net Ionic:
(10) half equation:
(11) half equation:
(12) Final Answer:
As2S5 + KNO3(aq) + HNO3(aq) à NO2 + H3AsO4(aq) + KHSO4(aq) + H2O
For additional Basic Media REDOX Homework-Ion Electron: (.25 points each)
(9) H2O2 + Cl2O7 + OH 1- à O2 + ClO21- + H2O
half equation:
half equation:
Final Answer:
H2O2 + Cl2O7 + OH 1- à O2 + ClO21- + H2O
------
(10) C4H4O62- + ClO31- + OH1- à CO3 2- + Cl1- + H2O
half equation:
half equation:
Final Answer:
C4H4O62- + ClO31- + OH1- à CO3 2- + Cl1- + H2O
(11) . Fe(CN)6 3- + Cr2O3 + OH 1- à Fe(CN)6 4- + CrO4 2- + H2O
half equation:
half equation:
Final Answer:
Fe(CN)6 3- + Cr2O3 + OH 1- à Fe(CN)6 4- + CrO4 2- + H2O
------
(12) BH4 1- + ClO31- à H2BO31- + Cl1- + H2O
half equation:
half equation:
Final Answer:
BH4 1- + ClO31- à H2BO31- + Cl1- + H2O
Basic Media Molecular Equation (0.50 Points Each)
(13)NaAlH4 (aq) + H2CO3 + NaCl(aq) + H2O à AlCl3 (aq) + CH3OH+ NaOH(aq)
Net Ionic:
(13) half equation:
(14) half equation:
(15) Final Answer:
NaAlH4 + H2CO3 + NaCl + H2O à AlCl3 + CH3OH + NaOH
------
(14) Na2CrO4 (aq) + Cu (s) + H2O à Cr(OH)3 (s) + Cu(OH)2(s) + NaOH (aq)
(16) Net Ionic:
(17) half equation:
(18) half equation:
Final Answer:
Na2CrO4 + Cu + H2O à Cr(OH)3 + Cu(OH)2 + NaOH