Table 7 Measured PH 4.0 4.11 4.0 12.00 4.90 HAC Ac HAC/Ac-4.0 Calculated pH 4.0 4.14 4.0 12.00 4.0 4.92 Enter a sample calculation for the experimental Ka for the 0.10 M NH4* solution and percent error. (The values you enter for your sample calculation should exactly match the corresponding values you entered above.) pH = -log[H*]; [H*] = 10-PH 4.0 (10-PH)² = (1 Ka [H+ ][A¯ ] [H+ 1² = [HA] = = 4.0✔ [HA] [HA] (0.10) 4.0 %error = lexperimental Ka value - literature K₂ value] literature Ka value x 100% = 4.0 % 10 x 100% = 4.0 4.0
Table 7 Measured PH 4.0 4.11 4.0 12.00 4.90 HAC Ac HAC/Ac-4.0 Calculated pH 4.0 4.14 4.0 12.00 4.0 4.92 Enter a sample calculation for the experimental Ka for the 0.10 M NH4* solution and percent error. (The values you enter for your sample calculation should exactly match the corresponding values you entered above.) pH = -log[H*]; [H*] = 10-PH 4.0 (10-PH)² = (1 Ka [H+ ][A¯ ] [H+ 1² = [HA] = = 4.0✔ [HA] [HA] (0.10) 4.0 %error = lexperimental Ka value - literature K₂ value] literature Ka value x 100% = 4.0 % 10 x 100% = 4.0 4.0
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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Transcribed Image Text:Table 7
Measured
PH
4.0
4.11
4.0 12.00
4.90
HAC
Ac
HAC/Ac-4.0
Calculated
pH
4.0
4.14
4.0 12.00
4.0 4.92
![Enter a sample calculation for the experimental Ka for the 0.10 M NH4* solution and percent error. (The values you enter for your sample calculation should exactly match the corresponding values you entered above.)
pH = -log[H*]; [H*] = 10-PH
4.0
(10-PH)² = (1
Ka
[H+ ][A¯ ] [H+ 1² =
[HA]
=
= 4.0✔
[HA]
[HA]
(0.10)
4.0
%error =
lexperimental Ka value - literature K₂ value]
literature Ka value
x 100% = 4.0
%
10
x 100% =
4.0
4.0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf0432bf-c1b5-433e-bde2-eaf9b9deba63%2F7f7c52db-9c63-4be5-a4a5-2cae3c2417c4%2F6cuuqfd_processed.png&w=3840&q=75)
Transcribed Image Text:Enter a sample calculation for the experimental Ka for the 0.10 M NH4* solution and percent error. (The values you enter for your sample calculation should exactly match the corresponding values you entered above.)
pH = -log[H*]; [H*] = 10-PH
4.0
(10-PH)² = (1
Ka
[H+ ][A¯ ] [H+ 1² =
[HA]
=
= 4.0✔
[HA]
[HA]
(0.10)
4.0
%error =
lexperimental Ka value - literature K₂ value]
literature Ka value
x 100% = 4.0
%
10
x 100% =
4.0
4.0
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