Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. NEXT > The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution. 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) 0.178 0.880-x [0] [0.888] [1.31 + x) 0 0 0.888 1.31 + x HC,H,Oz(aq) + [21.5] [x] Ka = 4.2 x 10-² 21.5 0.178 + x +x [37.7] [2x] 1 [0.178+x][0.888 + x] 37.7 -x 0.888 + x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 6.23 < PREV 1 2 NEXT > The Ka for HC₂H5O₂ is 6.3 x 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. [0.176] [21.5-x] H₂O(1) 2 pH = 0.176 4.37 21.5-x [0.261] [37.7 + x) 2 HạO*(aq) + C,H,Oz (aq) 0.261 37.7 + x = 6.3 x 10-5 2.4 x 10¹¹ [0.880] [0.176-x] 0.880 0.176-x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 7.77 [1.31] < PREV Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. [0.261 + x) 3 RESET 1.31 0.261 + x 9.63 RESET [0.178] [0.880 -x] RESET 0.880
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. NEXT > The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution. 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) 0.178 0.880-x [0] [0.888] [1.31 + x) 0 0 0.888 1.31 + x HC,H,Oz(aq) + [21.5] [x] Ka = 4.2 x 10-² 21.5 0.178 + x +x [37.7] [2x] 1 [0.178+x][0.888 + x] 37.7 -x 0.888 + x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 6.23 < PREV 1 2 NEXT > The Ka for HC₂H5O₂ is 6.3 x 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. [0.176] [21.5-x] H₂O(1) 2 pH = 0.176 4.37 21.5-x [0.261] [37.7 + x) 2 HạO*(aq) + C,H,Oz (aq) 0.261 37.7 + x = 6.3 x 10-5 2.4 x 10¹¹ [0.880] [0.176-x] 0.880 0.176-x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 7.77 [1.31] < PREV Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. [0.261 + x) 3 RESET 1.31 0.261 + x 9.63 RESET [0.178] [0.880 -x] RESET 0.880
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
![Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium
constant expression, and using this information to determine the pH. Complete Parts 1-3
before submitting your answer.
NEXT >
The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution.
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)
0.178
0.880-x
[0]
[0.888]
[1.31 + x)
0
0
0.888
1.31 + x
HC₂H5O₂(aq) +
[21.5]
[x]
Ka =
4.2 x 10-²
21.5
0.178 + x
+x
[37.7]
[2x]
1
[0.178+x][0.888 + x]
37.7
-x
0.888 + x
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium
constant expression, and using this information to determine the pH. Complete Parts 1-3
before submitting your answer.
6.23
< PREV
2
NEXT >
The Ka for HC₂H5O₂ is 6.3 x 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the
expression for Ka in order to determine the unknown. Each reaction participant must be represented by one
tile. Do not combine terms.
[0.176]
[21.5-x]
H₂O(1)
2
pH =
0.176
4.37
21.5-x
[0.261]
[37.7 + x)
2
HạO*(aq) + C,H,Oz (aq)
0.261
37.7 + x
= 6.3 x 10-5
2.4 x 10¹¹
[0.880]
[0.176-x]
0.880
0.176-x
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium
constant expression, and using this information to determine the pH. Complete Parts 1-3
before submitting your answer.
7.77
[1.31]
< PREV
Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the
buffer solution.
[0.261 + x)
3
RESET
1.31
0.261 + x
9.63
RESET
[0.178]
[0.880 -x]
RESET
0.880](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84d3fdf0-b73f-4040-a051-97beff994827%2Fe1dcf459-523d-45b0-8b2e-78e46817c304%2Fwsqk4n_processed.png&w=3840&q=75)
Transcribed Image Text:Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium
constant expression, and using this information to determine the pH. Complete Parts 1-3
before submitting your answer.
NEXT >
The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution.
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)
0.178
0.880-x
[0]
[0.888]
[1.31 + x)
0
0
0.888
1.31 + x
HC₂H5O₂(aq) +
[21.5]
[x]
Ka =
4.2 x 10-²
21.5
0.178 + x
+x
[37.7]
[2x]
1
[0.178+x][0.888 + x]
37.7
-x
0.888 + x
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium
constant expression, and using this information to determine the pH. Complete Parts 1-3
before submitting your answer.
6.23
< PREV
2
NEXT >
The Ka for HC₂H5O₂ is 6.3 x 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the
expression for Ka in order to determine the unknown. Each reaction participant must be represented by one
tile. Do not combine terms.
[0.176]
[21.5-x]
H₂O(1)
2
pH =
0.176
4.37
21.5-x
[0.261]
[37.7 + x)
2
HạO*(aq) + C,H,Oz (aq)
0.261
37.7 + x
= 6.3 x 10-5
2.4 x 10¹¹
[0.880]
[0.176-x]
0.880
0.176-x
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium
constant expression, and using this information to determine the pH. Complete Parts 1-3
before submitting your answer.
7.77
[1.31]
< PREV
Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the
buffer solution.
[0.261 + x)
3
RESET
1.31
0.261 + x
9.63
RESET
[0.178]
[0.880 -x]
RESET
0.880
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