Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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PROBLEM SOLVING 1 AND 2 ONLY
![logarithm of a ratio which can be solved by performing the antilogarithm of pH/pKa:
10pH-pKa [base]
An example of how to use the Henderson-Hasselbalch equation to solve for the pH of a buffer solution is as follows:
1.What is the pH of a buffer solution consisting of 0.0350 M NH3 and 0.0500 M NH4+ (Ka for NH4+ is 5.6 x 10-10)?
The equation for the reaction is:
NH+ H+ + NH3
Assuming that the change in concentrations is negligible, in order for the system to reach equilibrium, the Henderson-
Hasselbalch equation will be:
|NH:
%3D
['HN
0.0350
1301+vd = Hd
pH = 9.25 +log (
'0.0500
%3D
pH = 9.095
Activity3. True or False!
Directions: Write T if the statement is correct and F if otherwise. Write your answer before the number.
1. If the buffer is made with a base and its conjugate acid, the pH can be adjusted using a weak acid like HCl.
2. A buffer's pH changes greatly when a small amount of strong acid or base is added to it.
3. A good buffer mixture should have about equal concentrations of both of its components.
4. The strength of a weak acid (buffer) is usually represented as an equilibrium constant.
5.The Henderson-Hasselbalch equation connects the measurable value of the pH of a solution with the theoretical
value pKa.
Activity 4. It's Solving Time!
Directions: Solve the following problem. Write your complete solutions.
1. What is [H3O'] in a solution of 0.25 M CH3CO2H and 0.030 M NACH3CO2?
CH3CO2H(aq)+H2Om=H30°(aq)+CH3CO2 (ag)
2. What is [OH] in a solution of 0.125 M CH3NH, and 0.130 M CH3NH3CI?
CH3NH2(aq)+H2Ou=CH3NH3 (aq)+OH (aq)
K=1.8x105
(be)
Kp=4.4x10
(be)
Processing questions:
1. Why is understanding of the concept of pH important?
2. Why are buffer solutions relevant to life?
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Transcribed Image Text:logarithm of a ratio which can be solved by performing the antilogarithm of pH/pKa:
10pH-pKa [base]
An example of how to use the Henderson-Hasselbalch equation to solve for the pH of a buffer solution is as follows:
1.What is the pH of a buffer solution consisting of 0.0350 M NH3 and 0.0500 M NH4+ (Ka for NH4+ is 5.6 x 10-10)?
The equation for the reaction is:
NH+ H+ + NH3
Assuming that the change in concentrations is negligible, in order for the system to reach equilibrium, the Henderson-
Hasselbalch equation will be:
|NH:
%3D
['HN
0.0350
1301+vd = Hd
pH = 9.25 +log (
'0.0500
%3D
pH = 9.095
Activity3. True or False!
Directions: Write T if the statement is correct and F if otherwise. Write your answer before the number.
1. If the buffer is made with a base and its conjugate acid, the pH can be adjusted using a weak acid like HCl.
2. A buffer's pH changes greatly when a small amount of strong acid or base is added to it.
3. A good buffer mixture should have about equal concentrations of both of its components.
4. The strength of a weak acid (buffer) is usually represented as an equilibrium constant.
5.The Henderson-Hasselbalch equation connects the measurable value of the pH of a solution with the theoretical
value pKa.
Activity 4. It's Solving Time!
Directions: Solve the following problem. Write your complete solutions.
1. What is [H3O'] in a solution of 0.25 M CH3CO2H and 0.030 M NACH3CO2?
CH3CO2H(aq)+H2Om=H30°(aq)+CH3CO2 (ag)
2. What is [OH] in a solution of 0.125 M CH3NH, and 0.130 M CH3NH3CI?
CH3NH2(aq)+H2Ou=CH3NH3 (aq)+OH (aq)
K=1.8x105
(be)
Kp=4.4x10
(be)
Processing questions:
1. Why is understanding of the concept of pH important?
2. Why are buffer solutions relevant to life?
Page | 5
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