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⁺ <==========> NH₄¹⁺

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 OH^1-?

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 HSO₄^{1- is} a stronger acid than HPO₄^1- 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 1^st; 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:

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:

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:

Final Answer:

Zn + NO₃ ^1- + H ¹⁺ à Zn ²⁺ + NH₄ ¹⁺ + H₂O

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(4) Cr₂O₇ ^2- + C₂H₅OH + H ¹⁺ à Cr ³⁺ + HC₂H₃O₂ + H₂O

half equation:

Final Answer:

Cr₂O₇ ^2- + C₂H₅OH + H ¹⁺ à Cr ³⁺ + HC₂H₃O₂ + H₂O

(5) FeS + NO₃ ^1- + H ¹⁺ à NO + Fe ²⁺ + SO₄ ^2- + H₂O

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:

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:

Final Answer:

C₁₂H₂₂O₁₁ + H₂SO₄ + K₂Cr₂O₇ à CO₂ + Cr₂(SO₄)₃ + K₂SO₄+ H₂O

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(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+ ClO₂^1- + H₂O

half equation:

Final Answer:

H₂O₂ + Cl₂O₇+ OH ^1- à O₂+ ClO₂^1- + H₂O

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(10) C₄H₄O₆^2-+ ClO₃^1- + OH^1- à CO₃^2- + Cl^{1- +} H₂O

half equation:

Final Answer:

C₄H₄O₆^2-+ ClO₃^1- + OH^1- à CO₃^2- + Cl^{1- +} H₂O

(11) . Fe(CN)₆ ^3- + Cr₂O₃ + OH ^1- à Fe(CN)₆ ^4- + CrO₄ ^2- + H₂O

half equation:

Final Answer:

Fe(CN)₆ ^3- + Cr₂O₃ + OH ^1- à Fe(CN)₆ ^4- + CrO₄ ^2- + H₂O

-----------------------------------------------------------------

(12) BH₄ ^1- + ClO₃^1- à H₂BO₃^1- + Cl^1- + H₂O

half equation:

Final Answer:

BH₄ ^1- + ClO₃^1- à H₂BO₃^1- + Cl^1- + 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


Module 11i: Acids and Bases: A Molecular Look Jesperson Chapter 15	Possible	Actual
A. 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 concentrations Problems 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

(3) Zn + NO3 1- + H 1+ à Zn 2+ + NH4 1+ + H2O

Zn + NO3 1- + H 1+ à Zn 2+ + NH4 1+ + H2O

(9) H2O2 + Cl2O7 + OH 1- à O2 + ClO21- + H2O

(3) Zn + NO₃ ^1- + H ¹⁺ à Zn ²⁺ + NH₄ ¹⁺ + H₂O

Zn + NO₃ ^1- + H ¹⁺ à Zn ²⁺ + NH₄ ¹⁺ + H₂O

(9) H₂O₂ + Cl₂O₇+ OH ^1- à O₂+ ClO₂^1- + H₂O