A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. PREV 1 Based on your ICE table and definition of Ka, set up the expression for Ka and then evaluate it. Do not combine or simplify terms. Ka 5 RESET [0] [0.1000] [3.0] [0.030] [0.0030] [0.0970] [0.0097] [0.48] [2.5] 0.31 9.3 x 10 1.1 x 103 3.2 9.3 x 10
A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. PREV 1 Based on your ICE table and definition of Ka, set up the expression for Ka and then evaluate it. Do not combine or simplify terms. Ka 5 RESET [0] [0.1000] [3.0] [0.030] [0.0030] [0.0970] [0.0097] [0.48] [2.5] 0.31 9.3 x 10 1.1 x 103 3.2 9.3 x 10
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.72PAE
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![A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the
value of Ka for the weak acid.
PREV
1
m 2
Based on your ICE table and definition of Ka, set up the expression for Ka and then evaluate it.
Do not combine or simplify terms.
Ka
RESET
[0]
[0.1000]
[3.0]
[0.030]
[0.0030]
[0.0970]
[0.0097]
[0.48]
[2.5]
0.31
9.3 x 104
1.1 x 103
3.2
9.3 x 105](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3c12dbc-7691-49ef-84dd-9e94ae22700e%2Fdf33a70a-69c2-4c90-879e-d69589f70eb1%2Ft4hcqc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the
value of Ka for the weak acid.
PREV
1
m 2
Based on your ICE table and definition of Ka, set up the expression for Ka and then evaluate it.
Do not combine or simplify terms.
Ka
RESET
[0]
[0.1000]
[3.0]
[0.030]
[0.0030]
[0.0970]
[0.0097]
[0.48]
[2.5]
0.31
9.3 x 104
1.1 x 103
3.2
9.3 x 105
![A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the
value of Ka for the weak acid.
1
NEXT
Based on the given values, fill in the ICE table to determine concentrations of all reactants and
products.
HA(aq)
H,O(1)
H,O(aq)
A(aq)
+
Initial (M)
Change (M)
Equilibrium (M)
5 RESET
0.1000
3.0
-3.0
0.030
-0.030
0.0030
-0.0030
0.0970
-0.0970
0.0097
-0.0097](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3c12dbc-7691-49ef-84dd-9e94ae22700e%2Fdf33a70a-69c2-4c90-879e-d69589f70eb1%2Fftdi5nf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the
value of Ka for the weak acid.
1
NEXT
Based on the given values, fill in the ICE table to determine concentrations of all reactants and
products.
HA(aq)
H,O(1)
H,O(aq)
A(aq)
+
Initial (M)
Change (M)
Equilibrium (M)
5 RESET
0.1000
3.0
-3.0
0.030
-0.030
0.0030
-0.0030
0.0970
-0.0970
0.0097
-0.0097
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