C. Some Properties of Buffers Buffer system selected. NH4-NH3 HB is 1. pH of buffer 2. pH of diluted buffer 156 9.54 9.48 [H*]. [H*] NH4Cl CO.10 M) ? M pK, (by Eq. 4b) pK₁ 3. pH of buffer in which [HB]/[B] = 0.10 pH after addition of excess NaOH M Experiment 19 pH Measurements-Buffers and Their Properties (name the acid) 9.50. 10.54 11.83 pK₁
C. Some Properties of Buffers Buffer system selected. NH4-NH3 HB is 1. pH of buffer 2. pH of diluted buffer 156 9.54 9.48 [H*]. [H*] NH4Cl CO.10 M) ? M pK, (by Eq. 4b) pK₁ 3. pH of buffer in which [HB]/[B] = 0.10 pH after addition of excess NaOH M Experiment 19 pH Measurements-Buffers and Their Properties (name the acid) 9.50. 10.54 11.83 pK₁
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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Calculate H+ and pKa (given is pH) refer to the picture below. ANSWER ALL THE PART THAT HAS QUESTION MARK. PLEASE
Please include your solution.
PLEASE ANSWER QUESTIONS 1-3
and use the 2nd picture for the formula that must be used
![ammonium ion - ammonia
C. Some Properties of Buffers
Buffer system selected. NH4-NH3 HB is
1. pH of buffer
2. pH of diluted buffer
156
9.54
9.48
[H*].
[H*]
NH4Cl CO.10 M)
M pK, (by Eq. 4b)
M
pk,
?
Experiment 19 pH Measurements-Buffers and Their Properties
3. pH of buffer in which [HB]/[B] = 0.10
pH after addition of excess NaOH
(name the acid)
?
?
9.50.
10.54
11.83
pK₁](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fabb24741-0e22-4d20-9fa5-49d0725951c5%2F0f7eeb2c-678a-49b2-ad82-738d177be87a%2Fa17jcir_processed.jpeg&w=3840&q=75)
Transcribed Image Text:ammonium ion - ammonia
C. Some Properties of Buffers
Buffer system selected. NH4-NH3 HB is
1. pH of buffer
2. pH of diluted buffer
156
9.54
9.48
[H*].
[H*]
NH4Cl CO.10 M)
M pK, (by Eq. 4b)
M
pk,
?
Experiment 19 pH Measurements-Buffers and Their Properties
3. pH of buffer in which [HB]/[B] = 0.10
pH after addition of excess NaOH
(name the acid)
?
?
9.50.
10.54
11.83
pK₁
![a strong
The pH of such a buffer is established by the relative concentrations of HB and B in the solution. If we
manipulate Equation 4, we can solve for the concentration of H+ ion:
[H] = K₂ X [HB]/[B]
(4a)
This equation is often further modified when working with buffers, by taking the negative logarithm to base
10 of both sides:
pH pK,+ log [B]/[HB]
(4b)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fabb24741-0e22-4d20-9fa5-49d0725951c5%2F0f7eeb2c-678a-49b2-ad82-738d177be87a%2Fgmah9oh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:a strong
The pH of such a buffer is established by the relative concentrations of HB and B in the solution. If we
manipulate Equation 4, we can solve for the concentration of H+ ion:
[H] = K₂ X [HB]/[B]
(4a)
This equation is often further modified when working with buffers, by taking the negative logarithm to base
10 of both sides:
pH pK,+ log [B]/[HB]
(4b)
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