A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C¢H;NH2 is 3.8 x 10 10. ( PREV 1 2 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. 3.8 x 10-10 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5] [1.6 x 10-1º] [3.8 х 1010] [x + 4.20] [x - 4.20] [x + 6.3 x 10-5] [x - 6.3 x 10-1 [x + 1.6 x 10101 [x - 1.6 x 10-101 [x + 3.8 x 10101 [x - 3.8 x 1010]
A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C¢H;NH2 is 3.8 x 10 10. ( PREV 1 2 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. 3.8 x 10-10 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5] [1.6 x 10-1º] [3.8 х 1010] [x + 4.20] [x - 4.20] [x + 6.3 x 10-5] [x - 6.3 x 10-1 [x + 1.6 x 10101 [x - 1.6 x 10-101 [x + 3.8 x 10101 [x - 3.8 x 1010]
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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![A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI.
The initial concentration of C6H5NH2 is 0.50 M and the pH of the
buffer is 4.20. Determine the concentration of C6H5NH3* in the
solution. The value of Kb for C6H5NH2 is 3.8 x 10 10.
( PREV
1
3
NEXT >
Based on your ICE table and definition of Kb, set up the expression for Kb in
order to determine the unknown. Do not combine or simplify terms.
Kp
3.8 x 10-10
%3D
%3D
5 RESET
[0]
[0.50]
[x]
[2x]
[4.20]
[6.3 x 10-5)
[1.6 x 10-10]
[3.8 х
1011
[x + 4.20]
[x - 4.20]
[x + 6.3 x 10-51
[x - 6.3 х 10-5]
[x + 1.6 x 101°]
[x - 1.6 x 10-10]
[x + 3.8 x 10-101
[x - 3.8 x 101°]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5708a06e-b85b-454e-b228-7fe5c248a23c%2Faebabc27-2e5a-48f1-8e2d-9ce0b955fc70%2Flugow7o_processed.png&w=3840&q=75)
Transcribed Image Text:A buffer solution contains dissolved C6H5NH2 and C6H;NH3CI.
The initial concentration of C6H5NH2 is 0.50 M and the pH of the
buffer is 4.20. Determine the concentration of C6H5NH3* in the
solution. The value of Kb for C6H5NH2 is 3.8 x 10 10.
( PREV
1
3
NEXT >
Based on your ICE table and definition of Kb, set up the expression for Kb in
order to determine the unknown. Do not combine or simplify terms.
Kp
3.8 x 10-10
%3D
%3D
5 RESET
[0]
[0.50]
[x]
[2x]
[4.20]
[6.3 x 10-5)
[1.6 x 10-10]
[3.8 х
1011
[x + 4.20]
[x - 4.20]
[x + 6.3 x 10-51
[x - 6.3 х 10-5]
[x + 1.6 x 101°]
[x - 1.6 x 10-10]
[x + 3.8 x 10-101
[x - 3.8 x 101°]
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