Determine the Ka for a weak acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.017 0 0.002 HA(aq) 2.0 -0.002 0.030 0.011 H₂O(1) 0.013 -0.011 = 2 H_O(aq) 0.060 0.015 A (aq) RESET 0.017
Determine the Ka for a weak acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.017 0 0.002 HA(aq) 2.0 -0.002 0.030 0.011 H₂O(1) 0.013 -0.011 = 2 H_O(aq) 0.060 0.015 A (aq) RESET 0.017
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 2RQ: What is the law of mass action? Is it true that the value of K depends on the amounts of reactants...
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![< PREV
1
2
Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka. Each
reaction participant must be represented by one tile. Do not combine terms.
Once the expression is constructed, solve for the Ka of this weak acid.
[0]
[0.011]
[2.0]
3 x 10*
Ka
=
[0.030]
3 x 10³
[0.013]
7
[0.060]
0.2
=
[0.015]
[0.017]
RESET
[0.002]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3ea0963c-64ff-46a6-b97c-79944ef211ae%2F2e5951ec-44de-40e9-b70c-af8b37ae2da1%2F4rc13gn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:< PREV
1
2
Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka. Each
reaction participant must be represented by one tile. Do not combine terms.
Once the expression is constructed, solve for the Ka of this weak acid.
[0]
[0.011]
[2.0]
3 x 10*
Ka
=
[0.030]
3 x 10³
[0.013]
7
[0.060]
0.2
=
[0.015]
[0.017]
RESET
[0.002]
Transcribed Image Text:Determine the Ka for a weak acid by constructing an ICE table and using this
information to construct and solve the equilibrium constant expression. Complete
Parts 1-2 before submitting your answer.
1
NEXT >
0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium,
the concentration of HA was found to be 0.013 M. Fill in the ICE table with the appropriate value
for each involved species to determine the unknown concentrations of all reactants and products.
Initial (M)
Change (M)
Equilibrium (M)
-0.017
0
0.002
HA(aq)
2.0
-0.002
+
0.030
0.011
H₂O(1)
0.013
-0.011
=
2
H,O*(aq)
0.060
0.015
A (aq)
RESET
0.017
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