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 à base and its conjugate acid, the pH can be adjusted using a weak acid like HCI. 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.
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 à base and its conjugate acid, the pH can be adjusted using a weak acid like HCI. 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.
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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TRUE OR FALSE NUMBERS 1-5
![Tun pii amu kilown pRa, the solution of the Henderson-Hasselbalch equation gives the
logarithm of a ratio which can be solved by performing the antilogarithm of pH/pKa:
10pH-pKa [base]
Tacia
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:
INH
['HN
0.0350
1301+ vd = Hd
pH = 9.25+log (
0.0500
%3D
%3D
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 à 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 ofa solution with the theoretical
value pKa.
Activity 4. It's Solving Time!
Directions: Solve the following problem. Write your complete sohutions.
1. What is (H3Oʻ] in a solution of 0.25 M CH3CO,H and 0.030 M NACH3CO2?
CH3CO2H(aq)+H2Ou=H30°(aq)+CH3CO26
2. What is [OH] in a solution of 0.125 M CH3NH2 and 0.130 M CH3NH3CI?
CH3NH2(aq)+H2Ou CH3NH3 (aq)+OH (aq)
1. pH= pka + log
pH = 4.144 + log (O.12)
pH: 4.144 0-g2
PH= 3.924
K=1.8x105
(be)
K=4.4x104
[salt]
[Acid] = 4.744+ log_0.030M
2. poH = phot log alf 5.356t log 0.1uSM
0.130M
%3D
%3D
0.25M
Base I
%3D
PoH= 3.373
OLIQQ +954.€ =
[-HO I bo1- =Hod
Hod 9) = [-40k=
%3D
Therefore, [ H3o*]q0
Hd l = [,0Hk=
=X6H]=10-3.373
Processing questions. L500.0C014996M
- C#0]
[OH]= 4.236 y 10TM
%3D
1. Why is understanding of the concept of pH important?
The concept oF PH important For us to assist our body in creating and maintaining a
healthy pH ratio of 30 7:30, alkaline to acid. Most diseases, illness and bod bacteria
thrive in' an over
acidic environ ment
pog
2. Why are buffer solutions relevant to life?
BUFFer solutions relevant to life because
bibchemical processes
proceed
Also helps mointains
normally only when the PH remains within a Fairly narrow
a relatively constant pH in
a solution even in the Face
OF addition
OF acids or
Page | 5
bases](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6b275d4f-3298-41bf-bd83-0866b35786b7%2F2ccd0b20-ef94-460c-987a-657e26842627%2Fs4e0jjr.jpeg&w=3840&q=75)
Transcribed Image Text:Tun pii amu kilown pRa, the solution of the Henderson-Hasselbalch equation gives the
logarithm of a ratio which can be solved by performing the antilogarithm of pH/pKa:
10pH-pKa [base]
Tacia
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:
INH
['HN
0.0350
1301+ vd = Hd
pH = 9.25+log (
0.0500
%3D
%3D
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 à 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 ofa solution with the theoretical
value pKa.
Activity 4. It's Solving Time!
Directions: Solve the following problem. Write your complete sohutions.
1. What is (H3Oʻ] in a solution of 0.25 M CH3CO,H and 0.030 M NACH3CO2?
CH3CO2H(aq)+H2Ou=H30°(aq)+CH3CO26
2. What is [OH] in a solution of 0.125 M CH3NH2 and 0.130 M CH3NH3CI?
CH3NH2(aq)+H2Ou CH3NH3 (aq)+OH (aq)
1. pH= pka + log
pH = 4.144 + log (O.12)
pH: 4.144 0-g2
PH= 3.924
K=1.8x105
(be)
K=4.4x104
[salt]
[Acid] = 4.744+ log_0.030M
2. poH = phot log alf 5.356t log 0.1uSM
0.130M
%3D
%3D
0.25M
Base I
%3D
PoH= 3.373
OLIQQ +954.€ =
[-HO I bo1- =Hod
Hod 9) = [-40k=
%3D
Therefore, [ H3o*]q0
Hd l = [,0Hk=
=X6H]=10-3.373
Processing questions. L500.0C014996M
- C#0]
[OH]= 4.236 y 10TM
%3D
1. Why is understanding of the concept of pH important?
The concept oF PH important For us to assist our body in creating and maintaining a
healthy pH ratio of 30 7:30, alkaline to acid. Most diseases, illness and bod bacteria
thrive in' an over
acidic environ ment
pog
2. Why are buffer solutions relevant to life?
BUFFer solutions relevant to life because
bibchemical processes
proceed
Also helps mointains
normally only when the PH remains within a Fairly narrow
a relatively constant pH in
a solution even in the Face
OF addition
OF acids or
Page | 5
bases
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