(a) Calculate the [H30+] for each buffer solution and enter the value in Table D. Use the formula [H30+] = 10-pH, (Hint: The answer should contain two significant figures. This is the appropriate value when taking B.AA to the power of 10. The number of places after the decimal point, represented by A and A, determines the number of significant figures, Values before the decimal, represented by B, simply become part of the exponent of 10. So 10B.AA becomes .A x 108.) Table D: Calculation of Equilibrium Constant [BB"] from absorbance Measured absorbance at at v635 nm [HBB] from corrected Buffer [H30+] (a) Approximate Keg (c) pKeg (d) pH 470 nm absorbance at 470 nm (in-Lab Data Table C) (in-Lab Data Table C) (b) 6.30 4.0 4.0 49 40.1450 4 3528 4 .3238 5.0е-7 1.8e-7 4.0) 1.6e-7 6.80 4.0 4.0 403970 40.1866 4 .1072 2.3e-7 7.30 4.0 4.0 4.0 5.0e-7 4 .2362 4 2362 .1145 1.8e-7 too high Average pkeg (e) 4.0 Standard Deviation of pKeg (e) 4.0 Percent Standard Deviation of pKeg (e) 4.0 % (b) Reenter the measured absorbance at 635 nm from Table C of the lab. This is the [BB-), Reenter the measured absorbance at 470 nm from Table C of the Lab. Use the formula below to correct the absorbance at w470 nm and enter the calculated values in Table D as the [HBB]. (Additional Info) (HBB] = Absorbance470 - (0.2 x Absorbances35) %3D
(a) Calculate the [H30+] for each buffer solution and enter the value in Table D. Use the formula [H30+] = 10-pH, (Hint: The answer should contain two significant figures. This is the appropriate value when taking B.AA to the power of 10. The number of places after the decimal point, represented by A and A, determines the number of significant figures, Values before the decimal, represented by B, simply become part of the exponent of 10. So 10B.AA becomes .A x 108.) Table D: Calculation of Equilibrium Constant [BB"] from absorbance Measured absorbance at at v635 nm [HBB] from corrected Buffer [H30+] (a) Approximate Keg (c) pKeg (d) pH 470 nm absorbance at 470 nm (in-Lab Data Table C) (in-Lab Data Table C) (b) 6.30 4.0 4.0 49 40.1450 4 3528 4 .3238 5.0е-7 1.8e-7 4.0) 1.6e-7 6.80 4.0 4.0 403970 40.1866 4 .1072 2.3e-7 7.30 4.0 4.0 4.0 5.0e-7 4 .2362 4 2362 .1145 1.8e-7 too high Average pkeg (e) 4.0 Standard Deviation of pKeg (e) 4.0 Percent Standard Deviation of pKeg (e) 4.0 % (b) Reenter the measured absorbance at 635 nm from Table C of the lab. This is the [BB-), Reenter the measured absorbance at 470 nm from Table C of the Lab. Use the formula below to correct the absorbance at w470 nm and enter the calculated values in Table D as the [HBB]. (Additional Info) (HBB] = Absorbance470 - (0.2 x Absorbances35) %3D
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...
Related questions
Question
4
n the rest of the table? How do I solve the other blanks? This is from a post lab:
![(a) Calculate the [H30+] for each buffer solution and enter the value in Table D. Use the formula [H;0+] = 10-PH. (Hint: The answer should contain twvo significant
figures. This is the appropriate value when taking B.AA to the power of 10. The number of places after the decimal point, represented by A and A, determines the
number of significant figures, Values before the decimal, represented by B, simply become part of the exponent of 10. So 10B.AA becomes A.A x 1oB.)
Table D: Calculation of Equilibrium Constant
Buffer
Measured absorbance at
[H30+]
(a)
[BB"] from absorbance
at N635 nm
(in-Lab Data Table C)
[HBB] from corrected
absorbance at 470 nm
Approximate
Keg
(c)
pKeg
(d)
pH
N470 nm
(in-Lab Data Table C)
(ь)
6.30
4.0
4.0
4.0
.1450
4.0
49.3528
40.3238
5.0e-7
1.8e-7
6.80
4.0
4.0
4.0
40.3970
40.1866
40.1072
1.6e-7
2.3e-7
7.30
40
4.0
4.0
5.0e-7
4 .2362
40
.2362
1.1145
1.8e-7
too high
Average pkeg
(e)
Standard Deviation of pK eg
4.0
(e)
Percent Standard Deviation of pkeg
40
(e)
%
(b) Reenter the measured absorbance at 635 nm from Table C of the lab. This is the [BB-]. Reenter the measured absorbance at 470 nm from Table C of the Lab.
Use the formula below to correct the absorbance at 470 nm and enter the calculated values in Table D as the [HBB]. (Additional Info)
[HBB] = Absortance470 - (0.2 x Absorbance63s)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc5f81d2c-6cc2-4fbe-a7b6-26f56b17e4d5%2F725fc1d3-d509-48aa-89ca-abf3b66c3d4b%2F3w8wmjs_processed.jpeg&w=3840&q=75)
Transcribed Image Text:(a) Calculate the [H30+] for each buffer solution and enter the value in Table D. Use the formula [H;0+] = 10-PH. (Hint: The answer should contain twvo significant
figures. This is the appropriate value when taking B.AA to the power of 10. The number of places after the decimal point, represented by A and A, determines the
number of significant figures, Values before the decimal, represented by B, simply become part of the exponent of 10. So 10B.AA becomes A.A x 1oB.)
Table D: Calculation of Equilibrium Constant
Buffer
Measured absorbance at
[H30+]
(a)
[BB"] from absorbance
at N635 nm
(in-Lab Data Table C)
[HBB] from corrected
absorbance at 470 nm
Approximate
Keg
(c)
pKeg
(d)
pH
N470 nm
(in-Lab Data Table C)
(ь)
6.30
4.0
4.0
4.0
.1450
4.0
49.3528
40.3238
5.0e-7
1.8e-7
6.80
4.0
4.0
4.0
40.3970
40.1866
40.1072
1.6e-7
2.3e-7
7.30
40
4.0
4.0
5.0e-7
4 .2362
40
.2362
1.1145
1.8e-7
too high
Average pkeg
(e)
Standard Deviation of pK eg
4.0
(e)
Percent Standard Deviation of pkeg
40
(e)
%
(b) Reenter the measured absorbance at 635 nm from Table C of the lab. This is the [BB-]. Reenter the measured absorbance at 470 nm from Table C of the Lab.
Use the formula below to correct the absorbance at 470 nm and enter the calculated values in Table D as the [HBB]. (Additional Info)
[HBB] = Absortance470 - (0.2 x Absorbance63s)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY