E D C B 1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical A (aq) H.O*(aq) oll +
E D C B 1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical A (aq) H.O*(aq) oll +
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.58QE
Related questions
Question
![182
183
134
185
F
A
B
E
D
C
1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table
and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical
186
187
188
400
190
191
192
193
195
Reaction
Initial conc. / M:
Change in conc. at equilibrium
/M:
Equilibrium conc. / M:
pH
HA(aq) + H₂O(l)
0.1979
2.946990323
-2.2E-04
2. Use your data and the Henderson-Hasselbalch
pH=pka + log[A]/[HA] and
1.98E-01
Ka =
2.5E-07
pKa pH-log[A]/[HA]
=
pka
H3O*(aq)
0
5.9E+00
2.2E-04
2.2E-04
+
equation to perform the calculation and find Ka at any pH during titration.
Ka = 10 Ka
A (aq)
Ꮕ
Ka
2.2E-04
2.2E-04
1.3E-06
Hints:
Use Ex](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9513e069-36ff-4ceb-9003-aedf5c80ba1e%2F8f535efc-5b5a-49ee-a392-22836c1366de%2Ffnzo7xa_processed.jpeg&w=3840&q=75)
Transcribed Image Text:182
183
134
185
F
A
B
E
D
C
1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table
and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical
186
187
188
400
190
191
192
193
195
Reaction
Initial conc. / M:
Change in conc. at equilibrium
/M:
Equilibrium conc. / M:
pH
HA(aq) + H₂O(l)
0.1979
2.946990323
-2.2E-04
2. Use your data and the Henderson-Hasselbalch
pH=pka + log[A]/[HA] and
1.98E-01
Ka =
2.5E-07
pKa pH-log[A]/[HA]
=
pka
H3O*(aq)
0
5.9E+00
2.2E-04
2.2E-04
+
equation to perform the calculation and find Ka at any pH during titration.
Ka = 10 Ka
A (aq)
Ꮕ
Ka
2.2E-04
2.2E-04
1.3E-06
Hints:
Use Ex
Transcribed Image Text:pH 2.946990323
Comparison of Results:
pka
1 At 5.00 mL of NaOH before the equivalence point
2 At the equivalence point
3 At 5.00 ml after the equivalence point
5.9E+00
Ka
1.3E-06
LC POST-LAB QUESTIONS
These are OPTIONAL questions that can be used either as EC or as a substitute for the Module Quiz
Using experimentally determined values of Ka and molarity of your acid solution and the concentration of the standardized NaOH solution, calculate the pH
of the following points of your titration curve (check examples provided in the Lab Manual Manual):
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