Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3Cl and 0.500 M C6H5NH₂. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) 0.060 Initial (M) Change (M) Equilibrium (M) 0 -X 0.700 - x 1 -0.060 C6H5NH3*(aq) + OH (aq) 0 1 0.040 0.500 + x 0.140 0.300 + x 2 0.500 0.500 - x -0.040 0.300 - x -0.140 2 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 3 NEXT > Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. CoHsNHz(aq) + 0.100 0.500 H₂O(l) 0.020 0.100 + x 3 0.040 → H₂O(l) 0.100 - x -0.500 -0.020 4 0.100 0.700 0.040 + x + CoHsNHz(aq) RESET OH (aq) + C6H5NH3*(aq) 0.300 -0.100 0.040 - x RESET +x 0.700 + x
Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3Cl and 0.500 M C6H5NH₂. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) 0.060 Initial (M) Change (M) Equilibrium (M) 0 -X 0.700 - x 1 -0.060 C6H5NH3*(aq) + OH (aq) 0 1 0.040 0.500 + x 0.140 0.300 + x 2 0.500 0.500 - x -0.040 0.300 - x -0.140 2 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 3 NEXT > Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. CoHsNHz(aq) + 0.100 0.500 H₂O(l) 0.020 0.100 + x 3 0.040 → H₂O(l) 0.100 - x -0.500 -0.020 4 0.100 0.700 0.040 + x + CoHsNHz(aq) RESET OH (aq) + C6H5NH3*(aq) 0.300 -0.100 0.040 - x RESET +x 0.700 + x
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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Question
Transcribed Image Text:Determine the pH of a solution by constructing a BCA table, constructing an ICE table,
writing the equilibrium constant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
NEXT >
0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3Cl and 0.500 M
C6H5NH₂. Fill in the table with the appropriate value for each involved species to determine the moles of
reactant and product after the reaction of the acid and base. You can ignore the amount of water in the
reaction.
Before (mol)
Change (mol)
After (mol)
0.060
Initial (M)
Change (M)
Equilibrium (M)
0
-X
0.700 - x
1
-0.060
C6H5NH3*(aq) + OH (aq)
0
1
0.040
0.140
0.500 + x
CoHşNHz(aq) +
0.300 + x
2
0.500
0.500 - x
-0.040
0.300 - x
-0.140
Determine the pH of a solution by constructing a BCA table, constructing an ICE table,
writing the equilibrium constant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
2
< PREV
3
NEXT >
Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the
unknown concentrations of all reactants and products.
0.100
0.500
H₂O(l)
0.020
0.100 + x
3
0.040
→
H₂O(l)
0.100 - x
-0.500
-0.020
4
0.100
0.700
0.040 + x
+ CoHsNHz(aq)
RESET
OH (aq) + C6H5NH3*(aq)
0.300
-0.100
0.040 - x
RESET
+x
0.700 + x
![Determine the pH of a solution by constructing a BCA table, constructing an ICE table,
writing the equilibrium constant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
< PREV
1
2
3
NEXT >
The value of Kb for C6H5NH₂ is 4.3 x 10-10. Based on your ICE table (Part 2) 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.
[0]
[0.500 + x]
[0.300 + x]
0
[0.500]
[0.500 -x]
[0.300 -x]
0.200
Kb
[0.100]
[0.100 + x]
0.700
1.00 x 10-5 1.00 × 10-⁹
[0.040]
[0.100 -x]
2
Determine the pH of a solution by constructing a BCA table, constructing an ICE table,
writing the equilibrium constant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
pH
=
[0.700]
[0.040 + x]
< PREV
1
Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of
solution.
9.00
= 4.3 × 10-10
5.00
[0.300]
[0.040 -x]
3
20.7
[x]
[0.700 + x]
4
6.72
RESET
[0.700 -x]
[2x]
0.040
RESET](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84d3fdf0-b73f-4040-a051-97beff994827%2Fec577f38-6504-4fb0-a653-4bf4530c5053%2F5fufyx_processed.png&w=3840&q=75)
Transcribed Image Text:Determine the pH of a solution by constructing a BCA table, constructing an ICE table,
writing the equilibrium constant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
< PREV
1
2
3
NEXT >
The value of Kb for C6H5NH₂ is 4.3 x 10-10. Based on your ICE table (Part 2) 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.
[0]
[0.500 + x]
[0.300 + x]
0
[0.500]
[0.500 -x]
[0.300 -x]
0.200
Kb
[0.100]
[0.100 + x]
0.700
1.00 x 10-5 1.00 × 10-⁹
[0.040]
[0.100 -x]
2
Determine the pH of a solution by constructing a BCA table, constructing an ICE table,
writing the equilibrium constant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
pH
=
[0.700]
[0.040 + x]
< PREV
1
Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of
solution.
9.00
= 4.3 × 10-10
5.00
[0.300]
[0.040 -x]
3
20.7
[x]
[0.700 + x]
4
6.72
RESET
[0.700 -x]
[2x]
0.040
RESET
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