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. 1 3 4 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. 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. Before (mol) Change (mol) After (mol) -0.0075 Initial (M) Change (M) Equilibrium (M) E 0.313 - x 0 0.0100 0 0.500 + x 40.0 0.115 + x NH3(aq) -0.0100 NH3(aq) + 0.500 2 0.500 - x 0.115-x 0.500 2 0.0125 : on by constructing a BCA table, constructing an ICE table, ant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. -■· 0.300 + < PREV 1 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. 0.300 + x 25.0 H₂O(1) -0.0125 H*(aq) 0.192 0.300 0.300 - x 0.0200 0.300 - x -0.0200 0.313 0.192 + x 4 NH4*(aq) RESET OH(aq) + NH4* (aq) 0.115 0.0075 0.192 - x RESET +x 0.313 + 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. 1 3 4 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. 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. Before (mol) Change (mol) After (mol) -0.0075 Initial (M) Change (M) Equilibrium (M) E 0.313 - x 0 0.0100 0 0.500 + x 40.0 0.115 + x NH3(aq) -0.0100 NH3(aq) + 0.500 2 0.500 - x 0.115-x 0.500 2 0.0125 : on by constructing a BCA table, constructing an ICE table, ant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. -■· 0.300 + < PREV 1 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. 0.300 + x 25.0 H₂O(1) -0.0125 H*(aq) 0.192 0.300 0.300 - x 0.0200 0.300 - x -0.0200 0.313 0.192 + x 4 NH4*(aq) RESET OH(aq) + NH4* (aq) 0.115 0.0075 0.192 - x RESET +x 0.313 + x >
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.87QE
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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.
1
3
4
NEXT >
Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. 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.
Before (mol)
Change (mol)
After (mol)
-0.0075
Initial (M)
Change (M)
Equilibrium (M)
E
0.313 - x
0
0.0100
0
0.500 + x
40.0
0.115 + x
NH3(aq)
-0.0100
NH3(aq) +
0.500
2
0.500 - x
0.115-x
0.500
2
0.0125
:
on by constructing a BCA table, constructing an ICE table,
ant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
-■·
0.300
+
< PREV
1
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.
0.300 + x
25.0
H₂O(1)
-0.0125
H*(aq)
0.192
0.300
0.300 - x
0.0200
0.300 - x
-0.0200
0.313
0.192 + x
4
NH4*(aq)
RESET
OH(aq) + NH4* (aq)
0.115
0.0075
0.192 - x
RESET
+x
0.313 + 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
NEXT >
The value of Kb for NH3 is 1.8 x 10-5. 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]
[0.115 + x]
[0.500]
0
[0.500 -x]
0.693
[0.115-x]
Kb
=
3.00 x 10-5
[0.300]
[0.300 + x]
[0.192]
[0.300 -x]
10.41
3
pH =
[0.313]
3.32 x 10-1⁰
=
[0.192 + 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.
1.8 x 10-5
< PREV
1
2
Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of
solution.
4.52
3
4
[0.115]
[0.192 -x] [0.313 + x]
9.48
RESET
[2x]
0.500
[0.313 -x]
RESET
0.301](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84d3fdf0-b73f-4040-a051-97beff994827%2F23c73121-1366-4721-99c0-0f9d78dafcba%2Fzu8bhg7o_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
NEXT >
The value of Kb for NH3 is 1.8 x 10-5. 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]
[0.115 + x]
[0.500]
0
[0.500 -x]
0.693
[0.115-x]
Kb
=
3.00 x 10-5
[0.300]
[0.300 + x]
[0.192]
[0.300 -x]
10.41
3
pH =
[0.313]
3.32 x 10-1⁰
=
[0.192 + 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.
1.8 x 10-5
< PREV
1
2
Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of
solution.
4.52
3
4
[0.115]
[0.192 -x] [0.313 + x]
9.48
RESET
[2x]
0.500
[0.313 -x]
RESET
0.301
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