Kb for C6H5NH2 is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of C6H5NH3+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. C6H5NH2(aq) + H₂O(1) OH-(aq) + C6H5NH3+(aq) Initial (M) Change (M) Equilibrium (M) RESET 0 0.50 χ 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x - 4.20 x + 6.3 × 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10 PREV 1 2 3 NEXT Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = [0] [0.50] (x) [x +4.20] [x - 4.20] [x+6.3 x 10 < PREV 1 [2x] = 3.8 × 10-10 RESET [4.20] [6.3 x 10-5] [1.6 × 10-19] [3.8 × 10-19] [x-6.3 x 10] [x+1.6 × 10-9] [x-1.6 x 10-19 [x+3.8 x 10-9] [x-3.8 x 10-19 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the original concentration of C6H5NH3+. [C6H5NH3+] = M RESET 0 8.3 × 1010 0.86 1.2 10 2.1 0.50
Kb for C6H5NH2 is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of C6H5NH3+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. C6H5NH2(aq) + H₂O(1) OH-(aq) + C6H5NH3+(aq) Initial (M) Change (M) Equilibrium (M) RESET 0 0.50 χ 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x - 4.20 x + 6.3 × 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10 PREV 1 2 3 NEXT Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = [0] [0.50] (x) [x +4.20] [x - 4.20] [x+6.3 x 10 < PREV 1 [2x] = 3.8 × 10-10 RESET [4.20] [6.3 x 10-5] [1.6 × 10-19] [3.8 × 10-19] [x-6.3 x 10] [x+1.6 × 10-9] [x-1.6 x 10-19 [x+3.8 x 10-9] [x-3.8 x 10-19 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the original concentration of C6H5NH3+. [C6H5NH3+] = M RESET 0 8.3 × 1010 0.86 1.2 10 2.1 0.50
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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Transcribed Image Text:Kb for C6H5NH2 is 3.8 × 10-10. Complete Parts 1-3 before submitting your
answer.
1
2
3
NEXT >
A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of
C6H5NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the
original concentration of C6H5NH3+ in the water. Fill in the ICE table with the appropriate
value for each involved species to determine concentrations of all reactants and
products.
C6H5NH2(aq)
+
H₂O(1)
OH-(aq)
+
C6H5NH3+(aq)
Initial (M)
Change (M)
Equilibrium (M)
RESET
0
0.50
χ
4.20
-4.20
6.3 x 10-5
-6.3 x 10-5
1.6 × 10-10
-1.6 × 10-10
3.8 × 10-10
-3.8 × 10-10
x +4.20
x - 4.20
x + 6.3 × 10-5
x - 6.3 × 10-5
x + 1.6 × 10-10
x-1.6 × 10-10
x + 3.8 × 10-10
x - 3.8 × 10-10
![PREV
1
2
3
NEXT
Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in
order to determine the unknown. Each reaction participant must be represented by one
tile. Do not combine terms.
Kb =
[0]
[0.50]
(x)
[x +4.20]
[x - 4.20]
[x+6.3 x 10
< PREV
1
[2x]
=
3.8 × 10-10
RESET
[4.20]
[6.3 x 10-5]
[1.6 × 10-19]
[3.8 × 10-19]
[x-6.3 x 10] [x+1.6 × 10-9] [x-1.6 x 10-19 [x+3.8 x 10-9] [x-3.8 x 10-19
2
3
Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2),
determine the original concentration of C6H5NH3+.
[C6H5NH3+]
=
M
RESET
0
8.3 × 1010
0.86
1.2
10
2.1
0.50](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff922ab2d-c754-4c9c-9d3b-bd784fecfd89%2F95470506-9341-450b-846a-92d546aa6fb1%2Ff8td6tam_processed.png&w=3840&q=75)
Transcribed Image Text:PREV
1
2
3
NEXT
Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in
order to determine the unknown. Each reaction participant must be represented by one
tile. Do not combine terms.
Kb =
[0]
[0.50]
(x)
[x +4.20]
[x - 4.20]
[x+6.3 x 10
< PREV
1
[2x]
=
3.8 × 10-10
RESET
[4.20]
[6.3 x 10-5]
[1.6 × 10-19]
[3.8 × 10-19]
[x-6.3 x 10] [x+1.6 × 10-9] [x-1.6 x 10-19 [x+3.8 x 10-9] [x-3.8 x 10-19
2
3
Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2),
determine the original concentration of C6H5NH3+.
[C6H5NH3+]
=
M
RESET
0
8.3 × 1010
0.86
1.2
10
2.1
0.50
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