Determine the concentration of C.H.NH, in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the concentration of C.H.NH;*. Complete Parts 1-3 before submitting your answer. NEXT A buffer solution contains dissolved C.H.NH: and C.H.NH.CI. The initial concentration of C.H.NH: is 0.50 M and the pH of the buffer is 4.20. Let x represent the original concentration of CH:NH, in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 1.6 x 10 x+16 - 10 CcH:NH:(aq) -1.6 x 10 x-1.610 0.50 3.8 x 10 x+38-10 H:O(1) -3.8 x 10** x-3.8 -10 4.20 x +4.20 -4.20 x-4.20 OH (aq) 6.3 x 10* x+63-104 + CcH:NH, (aq) RESET -6.3 x 10* x-6.3*10*
Determine the concentration of C.H.NH, in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the concentration of C.H.NH;*. Complete Parts 1-3 before submitting your answer. NEXT A buffer solution contains dissolved C.H.NH: and C.H.NH.CI. The initial concentration of C.H.NH: is 0.50 M and the pH of the buffer is 4.20. Let x represent the original concentration of CH:NH, in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 1.6 x 10 x+16 - 10 CcH:NH:(aq) -1.6 x 10 x-1.610 0.50 3.8 x 10 x+38-10 H:O(1) -3.8 x 10** x-3.8 -10 4.20 x +4.20 -4.20 x-4.20 OH (aq) 6.3 x 10* x+63-104 + CcH:NH, (aq) RESET -6.3 x 10* x-6.3*10*
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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Can I please get help solving this question?
![Determine the concentration of C6H5NH3* in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of C6H5NH3Ť.
Complete Parts 1-3 before submitting your answer.
(
1
Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the original concentration of C6H5NH3+.
[C6H5NH3*]i
M
PREV
0
8.3 x 10¹⁰
0.86
2
=
1.2
10
2.1
3
RESET
0.50](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1a2e06cd-89b1-4949-854a-ccc1923a28fc%2F319a588b-45b0-4913-a19a-2b3a9245c50e%2Fe9olis_processed.png&w=3840&q=75)
Transcribed Image Text:Determine the concentration of C6H5NH3* in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of C6H5NH3Ť.
Complete Parts 1-3 before submitting your answer.
(
1
Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the original concentration of C6H5NH3+.
[C6H5NH3*]i
M
PREV
0
8.3 x 10¹⁰
0.86
2
=
1.2
10
2.1
3
RESET
0.50
![Determine the concentration of C«HsNH, in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of C.H.NH.*.
Complete Parts 1-3 before submitting your answer.
NEXT
A buffer solution contains dissolved C+HNH: and C&H:NH,CI. The initial concentration of CcHNH: is 0.50 M and the pH of the
buffer is 4.20. Let x represent the original concentration of C&H:NH, in the water. Fill in the ICE table with the appropriate value for
each involved species to determine concentrations of all reactants and products.
Initial (M)
Change (M)
Equilibrium (M)
1.6 x 10
x+1.6×10
CcH:NH:(aq)
0
[0]
[x+4.20]
-1.6 x 10⁰
x-1.6 10
0.50
3.8 x 10"
[0.50]
[x -4.20]
+
x+38*10*
Kb =
H:O(1)
[x]
-3.8 x 10-
[x+6.3 x 10
x-3.8*10*
4.20
x + 4.20
[2x]
[x-6.3 x 10
-4.20
x-4.20
Determine the concentration of C&HsNH, in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of CcHsNHst.
Complete Parts 1-3 before submitting your answer.
OH-(aq)
NEXT
2
PREV
The Kb for CcHsNH: is 3.8 x 10-10. 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.
[4.20]
[x+1.6 x 10
+
RESET
6.3 x 10*
x+6.3× 104 x-6.3 × 10*
= 3.8 x 10-10
CcH:NH,*(aq)
-6.3 x 10*
[x+3.8 x 10
RESET
[6.3 x 10] [1.6 x 10] [3.8 x 10
[x-1.6 x 10
[x-3.8 x 10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1a2e06cd-89b1-4949-854a-ccc1923a28fc%2F319a588b-45b0-4913-a19a-2b3a9245c50e%2Fo1zkr7v_processed.png&w=3840&q=75)
Transcribed Image Text:Determine the concentration of C«HsNH, in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of C.H.NH.*.
Complete Parts 1-3 before submitting your answer.
NEXT
A buffer solution contains dissolved C+HNH: and C&H:NH,CI. The initial concentration of CcHNH: is 0.50 M and the pH of the
buffer is 4.20. Let x represent the original concentration of C&H:NH, in the water. Fill in the ICE table with the appropriate value for
each involved species to determine concentrations of all reactants and products.
Initial (M)
Change (M)
Equilibrium (M)
1.6 x 10
x+1.6×10
CcH:NH:(aq)
0
[0]
[x+4.20]
-1.6 x 10⁰
x-1.6 10
0.50
3.8 x 10"
[0.50]
[x -4.20]
+
x+38*10*
Kb =
H:O(1)
[x]
-3.8 x 10-
[x+6.3 x 10
x-3.8*10*
4.20
x + 4.20
[2x]
[x-6.3 x 10
-4.20
x-4.20
Determine the concentration of C&HsNH, in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of CcHsNHst.
Complete Parts 1-3 before submitting your answer.
OH-(aq)
NEXT
2
PREV
The Kb for CcHsNH: is 3.8 x 10-10. 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.
[4.20]
[x+1.6 x 10
+
RESET
6.3 x 10*
x+6.3× 104 x-6.3 × 10*
= 3.8 x 10-10
CcH:NH,*(aq)
-6.3 x 10*
[x+3.8 x 10
RESET
[6.3 x 10] [1.6 x 10] [3.8 x 10
[x-1.6 x 10
[x-3.8 x 10
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Ok, so the system I am using for my homework said that my answer is wrong. This is the second time I asked a follow-up question in hopes I would get the corrected answer. The first follow-up question is still being reviewed. So I have attached what they said was wrong to this question in hopes that it might help solve the whole equation. Thank you
![Determine the concentration of C6H5NH3* in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of C6H5NH3*.
Complete Parts 1-3 before submitting your answer.
NEXT >
A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH₂ is 0.50 M and the pH 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.
Initial (M)
Change (M)
Equilibrium (M)
CoHsNHz(aq)
0.50
-1.6 x 10-¹⁰
0.50
+
2
H₂O(l)
OH-(aq)
0
3
x
1.6 x 10-1⁰
+
Incorrect, 1 attempt remaining
For this reaction, the Initial concentration for C6H5NH3* is non-zero. Your Initial concentration
for C6H5NH3+ is incorrect. Revisit the problem statement to determine the initial concentration
of acid or base. Also, make sure that your values are in the correct concentration units, not
mass or moles!
C6H5NH3+ (aq)
In this problem, the Change in concentration for OH- is known, so you should be able to
determine a number to represent the amount. Use the given pH to determine the
concentration of H3O+ or OH- at Equilibrium as appropriate. From there, you should be able to
determine the Change of each species, which is the difference between the Equilibrium and
Initial concentration. Recall that pH = -log([H3O+]) and that [H³O+][OH-] = 1 × 10-¹4
0
X
1.6 x 10-1⁰](https://content.bartleby.com/qna-images/question/1a2e06cd-89b1-4949-854a-ccc1923a28fc/ecb78658-4fba-4111-8d6f-2755c4071b1f/86qu3tw_processed.png)
Transcribed Image Text:Determine the concentration of C6H5NH3* in a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the concentration of C6H5NH3*.
Complete Parts 1-3 before submitting your answer.
NEXT >
A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH₂ is 0.50 M and the pH 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.
Initial (M)
Change (M)
Equilibrium (M)
CoHsNHz(aq)
0.50
-1.6 x 10-¹⁰
0.50
+
2
H₂O(l)
OH-(aq)
0
3
x
1.6 x 10-1⁰
+
Incorrect, 1 attempt remaining
For this reaction, the Initial concentration for C6H5NH3* is non-zero. Your Initial concentration
for C6H5NH3+ is incorrect. Revisit the problem statement to determine the initial concentration
of acid or base. Also, make sure that your values are in the correct concentration units, not
mass or moles!
C6H5NH3+ (aq)
In this problem, the Change in concentration for OH- is known, so you should be able to
determine a number to represent the amount. Use the given pH to determine the
concentration of H3O+ or OH- at Equilibrium as appropriate. From there, you should be able to
determine the Change of each species, which is the difference between the Equilibrium and
Initial concentration. Recall that pH = -log([H3O+]) and that [H³O+][OH-] = 1 × 10-¹4
0
X
1.6 x 10-1⁰
Solution
by Bartleby ExpertFollow-up Question
Thank you that was helpful. I am having trouble with what to put into the Ice table. I got the same answer as you but not all those answers are available to choose from.
Solution
by Bartleby ExpertKnowledge Booster
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