1. Using initial molarity of acid and measured pH of the acid before titration, build a RICE table and calculate the Ka of the acid. You can use examples 1, 2 (pp. 3-4) from the Manual (posted on Canvas) Initial Molarity of [HA], M 0.219 Initial pH of Acid 3.20 Reaction Initial conc. / M: Change in conc. at equilibrium / M: Equilibrium conc. / M: 2. Ka = HA(aq) + H₂O(1) [HA] pka = -X [HA] + x H3O+(aq) 0 pH = +X +X Use the Henderson-Hasselbauch equation to perform the same calculation. Ka = + [H3O+] [A-] [HA] [H+] = A-(aq) 0 +X +X 6.3E-04 pH = pka + log[A-]/[HA]
1. Using initial molarity of acid and measured pH of the acid before titration, build a RICE table and calculate the Ka of the acid. You can use examples 1, 2 (pp. 3-4) from the Manual (posted on Canvas) Initial Molarity of [HA], M 0.219 Initial pH of Acid 3.20 Reaction Initial conc. / M: Change in conc. at equilibrium / M: Equilibrium conc. / M: 2. Ka = HA(aq) + H₂O(1) [HA] pka = -X [HA] + x H3O+(aq) 0 pH = +X +X Use the Henderson-Hasselbauch equation to perform the same calculation. Ka = + [H3O+] [A-] [HA] [H+] = A-(aq) 0 +X +X 6.3E-04 pH = pka + log[A-]/[HA]
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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![Unknown Acid
Acid name
Acetic acid
Group #5
Group #6
Group #7
Mean
Standard Deviation
% Error
STATISTICAL ANALYSIS: Calculate mean values for molar mass, pKa, and Ka. Calculate % error and standard deviation:
Unknown acid # 1
Molar Mass of unknown acid (calculated), g/mol
Group #1
Group #2
Group #3
Group #4
Reaction
Initial conc. / M:
Change in conc. at
equilibrium / M:
Equilibrium conc. / M:
Acetic acid | Molar Mass, g/mol: 60.05 | pka = 4.76
Accepted Values
Molar mass, g/mol
60.05
Ka =
Part II
1. Using initial molarity of acid and measured pH of the acid before titration, build a RICE table and
calculate the Ka of the acid. You can use examples 1, 2 (pp. 3-4) from the Manual (posted on Canvas)
Initial Molarity of [HA], M
0.219
Initial pH of Acid
pka =
HA(aq) + H₂O(1)
[HA]
-X
58.8
57.4
60.4
61.0
58.4
59.2
59.7
59.3
1.13
0.01
[HA] + X
台
pH:
H3O+ (aq)
=
0
+X
2. Use the Henderson-Hasselbauch equation to perform the same calculation.
+X
pka
4.76
Ka =
pka
4.78
5.00
4.64
4.89
4.62
4.68
4.82
4.78
0.13
0.42
3.20
[H3O+] [A-]
[HA]
[H+] =
A-(aq)
0
+X
Ka
1.74E-05
+X
Ka
1.66E-05
1.00E-05
2.29E-05
1.29E-05
2.40E-05
2.09E-05
1.74E-05
1.78E-05
0.00
0.6
6.3E-04
pH = pka + log[A-]/[HA]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F96023f4d-6281-4c81-803e-adfe3e4197d6%2Ff1666302-4bda-4125-844d-a92dd2b6d51f%2F3bz6cfd_processed.png&w=3840&q=75)
Transcribed Image Text:Unknown Acid
Acid name
Acetic acid
Group #5
Group #6
Group #7
Mean
Standard Deviation
% Error
STATISTICAL ANALYSIS: Calculate mean values for molar mass, pKa, and Ka. Calculate % error and standard deviation:
Unknown acid # 1
Molar Mass of unknown acid (calculated), g/mol
Group #1
Group #2
Group #3
Group #4
Reaction
Initial conc. / M:
Change in conc. at
equilibrium / M:
Equilibrium conc. / M:
Acetic acid | Molar Mass, g/mol: 60.05 | pka = 4.76
Accepted Values
Molar mass, g/mol
60.05
Ka =
Part II
1. Using initial molarity of acid and measured pH of the acid before titration, build a RICE table and
calculate the Ka of the acid. You can use examples 1, 2 (pp. 3-4) from the Manual (posted on Canvas)
Initial Molarity of [HA], M
0.219
Initial pH of Acid
pka =
HA(aq) + H₂O(1)
[HA]
-X
58.8
57.4
60.4
61.0
58.4
59.2
59.7
59.3
1.13
0.01
[HA] + X
台
pH:
H3O+ (aq)
=
0
+X
2. Use the Henderson-Hasselbauch equation to perform the same calculation.
+X
pka
4.76
Ka =
pka
4.78
5.00
4.64
4.89
4.62
4.68
4.82
4.78
0.13
0.42
3.20
[H3O+] [A-]
[HA]
[H+] =
A-(aq)
0
+X
Ka
1.74E-05
+X
Ka
1.66E-05
1.00E-05
2.29E-05
1.29E-05
2.40E-05
2.09E-05
1.74E-05
1.78E-05
0.00
0.6
6.3E-04
pH = pka + log[A-]/[HA]
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