CHM 2046C Module Eleven-Chapter 14 Name:____________

 

Module Eleven: Acid/Base Equilibria McMurry Chapter 14

Possible

Actual

A. Idenification of Bronsted-Lowry/Lewis acids&bases

10

 

B. Writing Equilibrium Constant Expressions

10

 

C. Determination of Kw from Kc ; Kb from Ka & Kw ; Show Kb x Ka = Kw Lecture

10

 

D. Determination of pH & pOH from concentrations Problems

10

 

E. Determination of pH of weak acids/bases Problems

10

 

F. Hydrolysis Reactions 

10

 

G. Common Ion Effect Problem

10

 

H. Discussion Questions Chapter 14

5

 

I. Determination of pH of polyprotic acids and/or Buffer Calculation Problem

10

 

J. Acid-Base Properties of Salts

10

 

K. Key Terms Chapter 14

10

 

M. Multiple Choice Applications -Chapter 14

25

 

Total: 130

Part A: Identification of Acids and Bases 10 points

Label the acid and the base and their corresponding conjugate 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

 

 

 

 

 

 

 


 

CHEM 1212 M-11 Sample Exam

Part B: Equilibrium Constant Expressions of Acids and Bases 5 points

Write the appropriate equilibrium constant expressions for the following reactions they represent:

 

a. C5H5NH+1 + H2O C5H5N + H3O+1

 

 

 

Ka =

 

 

b. NH3 + H2O NH4 1+ + OH 1-

 

 

 

Kb =

 

 

c.                   H2CO3 + H2O = HCO3 1- + H3O+1

 

 

 

Ka =

 

 

 

d. HCO3 1- + H2O == CO3 2- + H3O+1

 

 

 

Ka2 =

 

 

 

 

 

e. C5H5N + H2O ==== + OH 1- + C5H5N+1

 

 

Kb =

 

 

 

f. H2O + H2O == H3O 1+ + OH 1-

 

Kw =