Determine the pH of a solution of aspirin (acetylsalicylic acid, HC,H7O4) by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of aspirin is 3.3 × 104. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT 652 mg of aspirin (HC9H7O4) is dissolved in an aqueous solution of 237 mL aqueous solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HC9H7O4(aq) + H₂O(1) Initial (M) Change (M) Equilibrium (M) ☐ 0 = H3O+(aq) + C9H7O4(aq) 2.75 x 10-3 3.62 × 10-3 1.53 x 10-5 15.3 0.0153 RESET +x -x 2.75 x 10-3 + x 2.75 x 10-3-X 3.62 x 10-3 + x 3.62 x 10-3-X 1.53 x 10-5 + X 1.53 x 10-5-x 15.3 + x 15.3 - x 0.0153 + x 0.0153 - x < PREV 1 2 3 NEXT > Based on your ICE table 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] Ka = [2.75 x 10-3] [3.62 x 10-3] [1.53 x 10-5] [15.3] = 3.3 × 10-4 [0.0153] [2.75 x 10³ + x] [2.75 x 10-x] [3.62 x 103+x] [3.62 x 103 - x] [1.53 x 105+x] [1.53 x 10-5 - x] [0.0153 + x] [0.0153 - x] < PREV 2 3 RESET [x] [2x] [15.3 + x] [15.3-x] Based on your ICE table and the equilibrium expression for Ka, determine the pH of the aspirin solution. pH = RESET 0 6.17 2.25 x 10-³ 2.09 × 10-3 2.68 5.05 x 10-5 5.30 12.2
Determine the pH of a solution of aspirin (acetylsalicylic acid, HC,H7O4) by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of aspirin is 3.3 × 104. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT 652 mg of aspirin (HC9H7O4) is dissolved in an aqueous solution of 237 mL aqueous solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. HC9H7O4(aq) + H₂O(1) Initial (M) Change (M) Equilibrium (M) ☐ 0 = H3O+(aq) + C9H7O4(aq) 2.75 x 10-3 3.62 × 10-3 1.53 x 10-5 15.3 0.0153 RESET +x -x 2.75 x 10-3 + x 2.75 x 10-3-X 3.62 x 10-3 + x 3.62 x 10-3-X 1.53 x 10-5 + X 1.53 x 10-5-x 15.3 + x 15.3 - x 0.0153 + x 0.0153 - x < PREV 1 2 3 NEXT > Based on your ICE table 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] Ka = [2.75 x 10-3] [3.62 x 10-3] [1.53 x 10-5] [15.3] = 3.3 × 10-4 [0.0153] [2.75 x 10³ + x] [2.75 x 10-x] [3.62 x 103+x] [3.62 x 103 - x] [1.53 x 105+x] [1.53 x 10-5 - x] [0.0153 + x] [0.0153 - x] < PREV 2 3 RESET [x] [2x] [15.3 + x] [15.3-x] Based on your ICE table and the equilibrium expression for Ka, determine the pH of the aspirin solution. pH = RESET 0 6.17 2.25 x 10-³ 2.09 × 10-3 2.68 5.05 x 10-5 5.30 12.2
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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Transcribed Image Text:Determine the pH of a solution of aspirin (acetylsalicylic acid, HC,H7O4)
by constructing an ICE table, writing the equilibrium constant expression,
and using this information to determine the pH. The Ka of aspirin is 3.3 ×
104. Complete Parts 1-3 before submitting your answer.
1
2
3
NEXT
652 mg of aspirin (HC9H7O4) is dissolved in an aqueous solution of 237 mL aqueous
solution. Fill in the ICE table with the appropriate value for each involved species to
determine concentrations of all reactants and products.
HC9H7O4(aq)
+
H₂O(1)
Initial (M)
Change (M)
Equilibrium (M)
☐
0
=
H3O+(aq)
+
C9H7O4(aq)
2.75 x 10-3
3.62 × 10-3
1.53 x 10-5
15.3
0.0153
RESET
+x
-x
2.75 x 10-3 + x
2.75 x 10-3-X
3.62 x 10-3 + x
3.62 x 10-3-X
1.53 x 10-5 + X
1.53 x 10-5-x
15.3 + x
15.3 - x
0.0153 + x
0.0153 - x
![< PREV
1
2
3
NEXT >
Based on your ICE table 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]
Ka
=
[2.75 x 10-3]
[3.62 x 10-3] [1.53 x 10-5]
[15.3]
= 3.3 × 10-4
[0.0153]
[2.75 x 10³ + x] [2.75 x 10-x] [3.62 x 103+x] [3.62 x 103 - x] [1.53 x 105+x] [1.53 x 10-5 - x]
[0.0153 + x]
[0.0153 - x]
< PREV
2
3
RESET
[x]
[2x]
[15.3 + x]
[15.3-x]
Based on your ICE table and the equilibrium expression for Ka, determine the pH of the
aspirin solution.
pH =
RESET
0
6.17
2.25 x 10-³
2.09 × 10-3
2.68
5.05 x 10-5
5.30
12.2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff922ab2d-c754-4c9c-9d3b-bd784fecfd89%2F854b23b0-eed6-4e01-af9c-0168d3930e63%2Fm4pl4v_processed.png&w=3840&q=75)
Transcribed Image Text:< PREV
1
2
3
NEXT >
Based on your ICE table 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]
Ka
=
[2.75 x 10-3]
[3.62 x 10-3] [1.53 x 10-5]
[15.3]
= 3.3 × 10-4
[0.0153]
[2.75 x 10³ + x] [2.75 x 10-x] [3.62 x 103+x] [3.62 x 103 - x] [1.53 x 105+x] [1.53 x 10-5 - x]
[0.0153 + x]
[0.0153 - x]
< PREV
2
3
RESET
[x]
[2x]
[15.3 + x]
[15.3-x]
Based on your ICE table and the equilibrium expression for Ka, determine the pH of the
aspirin solution.
pH =
RESET
0
6.17
2.25 x 10-³
2.09 × 10-3
2.68
5.05 x 10-5
5.30
12.2
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