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
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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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