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
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
Problem 70AP
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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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