A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 3 A 50.0 mL solution of 0.300 M CH3COOH was titrated with 0.300 M NaOH. 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) 0.150 Initial (M) Change (M) Equilibrium (M) 0.0150 - x CH3COOH(aq) + OH (aq) 0 -0.150 0 1 0.150 -0.150 0.300+ x 0 0.0200 + x 0.300 CH3COO (aq) + 0.0150 0.150 -X 2 0.150 - x 0.300 0.300 - x 0.0200 - x -0.300 -0.0150 2 0.150 A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. -0.150 0.0300 0 < PREV Upon completion of the acid-base reaction, the acetate ion (CH3COO) is in equilibrium with water. Set up the ICE table in order to determine the unknown concentrations of reactants and products.. 15.0 H₂O(l) 0.0300 + x 50.0 0.150 H₂O(l) 3 -15.0 0.0300 x -50.0 0.0150 4 OH (aq) 0 +X +x 0.0300 0.150 + x NEXT + CH3COO (aq) 4 0 0.150 0.0200 0.150-x 0.150 RESET -0.0300 + CH3COOH(aq) 0 NEXT +X > +X RESET +x 0.0150 + x
A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 3 A 50.0 mL solution of 0.300 M CH3COOH was titrated with 0.300 M NaOH. 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) 0.150 Initial (M) Change (M) Equilibrium (M) 0.0150 - x CH3COOH(aq) + OH (aq) 0 -0.150 0 1 0.150 -0.150 0.300+ x 0 0.0200 + x 0.300 CH3COO (aq) + 0.0150 0.150 -X 2 0.150 - x 0.300 0.300 - x 0.0200 - x -0.300 -0.0150 2 0.150 A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. -0.150 0.0300 0 < PREV Upon completion of the acid-base reaction, the acetate ion (CH3COO) is in equilibrium with water. Set up the ICE table in order to determine the unknown concentrations of reactants and products.. 15.0 H₂O(l) 0.0300 + x 50.0 0.150 H₂O(l) 3 -15.0 0.0300 x -50.0 0.0150 4 OH (aq) 0 +X +x 0.0300 0.150 + x NEXT + CH3COO (aq) 4 0 0.150 0.0200 0.150-x 0.150 RESET -0.0300 + CH3COOH(aq) 0 NEXT +X > +X RESET +x 0.0150 + x
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section: Chapter Questions
Problem 35PS: Using Figure 17.11, suggest an indicator to use in each of the following titrations: (a) The weak...
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![A student was titrating a solution of acetic acid with a sodium hydroxide solution.
Determine the pH at the equivalence point. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
PREV
1
2
3
NEXT >
The Ka for CH3COOH is 1.8 x 10-5. Based on your ICE table and the equilibrium expression for Kb, set up
the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be
represented by one tile. Do not combine terms.
[0]
[0.300 -x]
1.8 x 10-²
[0.300]
0
[0.0300 + x]
5.6 x 10-1⁰
2.75
Kb =
[0.0300]
[0.0300 -x]
5.6 x 10-8
1.30 x 10-5
5.04
[x]
0.523
[0.150 -x]
8.96
[0.150]
[0.150 + x]
2
[x]
A student was titrating a solution of acetic acid with a sodium hydroxide solution.
Determine the pH at the equivalence point. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
pH =
< PREV
1
3
4
Based on your ICE table and the equilibrium expression for Kb, determine the pH of this solution at the
equivalence point..
1.20
[0.0150]
[0.150 -x] [0.0150 + x]
5.6 x 10-1⁰
8.96
[x]
7.72 x 10-1⁰
4
[2x]
4.89
[0.0150 -x]
RESET
[0.300 + x]
1.8 x 10-5
11.3
RESET
9.11](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84d3fdf0-b73f-4040-a051-97beff994827%2Feafae7c5-1705-4434-a5f1-44190db26313%2F70n2cmv_processed.png&w=3840&q=75)
Transcribed Image Text:A student was titrating a solution of acetic acid with a sodium hydroxide solution.
Determine the pH at the equivalence point. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
PREV
1
2
3
NEXT >
The Ka for CH3COOH is 1.8 x 10-5. Based on your ICE table and the equilibrium expression for Kb, set up
the expression for Kb in order to determine the unknown concentrations. Each reaction participant must be
represented by one tile. Do not combine terms.
[0]
[0.300 -x]
1.8 x 10-²
[0.300]
0
[0.0300 + x]
5.6 x 10-1⁰
2.75
Kb =
[0.0300]
[0.0300 -x]
5.6 x 10-8
1.30 x 10-5
5.04
[x]
0.523
[0.150 -x]
8.96
[0.150]
[0.150 + x]
2
[x]
A student was titrating a solution of acetic acid with a sodium hydroxide solution.
Determine the pH at the equivalence point. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
pH =
< PREV
1
3
4
Based on your ICE table and the equilibrium expression for Kb, determine the pH of this solution at the
equivalence point..
1.20
[0.0150]
[0.150 -x] [0.0150 + x]
5.6 x 10-1⁰
8.96
[x]
7.72 x 10-1⁰
4
[2x]
4.89
[0.0150 -x]
RESET
[0.300 + x]
1.8 x 10-5
11.3
RESET
9.11
Transcribed Image Text:A student was titrating a solution of acetic acid with a sodium hydroxide solution.
Determine the pH at the equivalence point. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
3
A 50.0 mL solution of 0.300 M CH3COOH was titrated with 0.300 M NaOH. 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)
0.150
Initial (M)
Change (M)
Equilibrium (M)
0.0150 - x
CH3COOH(aq) + OH (aq)
0
-0.150
0
1
0.150
-0.150
0.300+ x
0
0.0200 + x
0.300
CH3COO (aq) +
0.0150
0.150
-X
2
0.150 - x
0.300
0.300 - x
0.0200 - x
-0.300
-0.0150
2
0.150
A student was titrating a solution of acetic acid with a sodium hydroxide solution.
Determine the pH at the equivalence point. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
-0.150
0.0300
0
< PREV
Upon completion of the acid-base reaction, the acetate ion (CH3COO) is in equilibrium with water. Set up
the ICE table in order to determine the unknown concentrations of reactants and products..
15.0
H₂O(l)
0.0300 + x
50.0
0.150
H₂O(l)
3
-15.0
0.0300 x
-50.0
0.0150
4
OH (aq)
0
+X
+x
0.0300
0.150 + x
NEXT
+ CH3COO (aq)
4
0
0.150
0.0200
0.150-x
0.150
RESET
-0.0300
+ CH3COOH(aq)
0
NEXT
+X
>
+X
RESET
+x
0.0150 + x
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