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 AnswerB. Idenitication of Lewis Acids and Bases – Section 15.4 1C. Writing Ionization Reactions Strong/Weak Arrhenius Acid/Bases Section 4.4 1 AnswersC1. Strengths of Bronsted-Lowry Acids and Bases – Section 15.2 1C2. Periodic Trends in Strengths of Acids – Section 15.3 1D. Determination of pH & pOH from concentrations   Problems Section 16.1 2 AnswerD. pH Sample 2   AnswerW. Rewriting Equations Ionically Section 4.8 5 Answers

Answer Explained AnswerR. 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 pointLabel 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 15.1Look 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 736Try 15.5 and 15.6 page 737 Review Question 15.1-15.5 Page 758Try ReviewProblesm 15.49-15.54 Pages 759-760Answers: http://www.fccj.us/chm2046/SampleTest/46M11abAnswer.htm

CHM 2046C Module 11i Homework PacketPart B: Identification of Lewis Acids and Bases 1 pointDraw 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 7.4Try Practice Exercises 15.17 and 15.18 Page 749Look at Review Questions 15.25-15.32 Page 759Try Review Problems 15.61-15.68 Page 760

CHM 2046C Module 11i Homework PacketPart 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 4.4Try Practice 4.5 and 4.6 Page 167Look at Example 4.3 page169; Try Practice 4.7 and 4.8 Page 169Look at Example 5.4 Page 171 Try Practice 4.9 and 4.10 Page 171Answer Review Questions 4.13-4.25 Page 205 Review Problems 4.51-4.60 Page 207CHM 2046C Module 11i Homework Packet

Part C1 Strengths of Bronsted-Lowry Acids and Bases: 1 Point1. 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 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 15.2Look at Example 15.3 page 740Try Practice Exercise15.7 and 15.8 page 741Try Review Questions 15.6-15.13 page 758Try 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 15.3Look at Tables 15.1 Page 741 and Table 15.2 Page 742Try Practice Exercise15.9 and 15.10 page 742Try Practice Exercise15.11 and 15.12 page 744Try Practice Exercise15.13 and 15.14 page 745Try Review Questions 15.14-15.15 page 758Try Review Problems 15.55-15.60 page 760

CHM 2046C Module 11i Homework PacketPart 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 16.2Try Practice 16.1 and 16.2 Page 765Try Practice 16.3, 16.4, and 16.5 Page 767Try Practice 16.6 and 16.7 Page 768Answer Review Questions 16.8-16.13 Pages 808-809Review Problems 16.49-16.62 Page 810 Answers: http://www.fccj.us/chm2046/SampleTest/46M11dAnswer.htm

CHM 2046C Module 11i Homework PacketModule 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 4.3Look at Example 4.2 Page 162Try Practice 4.3 and 4.4 Page 163Look at Review Questions 4.11 and 4.12 Page 205Try Review Problems 4.47-4.50 Page 206Answers 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 pointsYour 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 MethodLook at Example 5.5 page 223 Try Practice 5.7 and 5.8 Page 224Online REDOX Study Guide: http://www.fscj.me/REDOX/REDOXstudy.html Look at Review Questions 5.6-5.10Review Problems: 5.43-5.48 Pages 243-244Some 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- + ClO3

1- + OH1- à CO3 2- + Cl1- + H2O

half equation:

 

 

   

half equation:

 

  

 

 Final Answer:

C4H4O62- + ClO3

1- + 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 H2BO3

1- + Cl1- + H2O

half equation:

 

   

half equation:

 

 

 

 Final Answer:

BH4 1- + ClO31- à H2BO3

1- + 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