A 15.00 ml aliquot of a 0.75 M solution of a weak acid (Ka = 1.50E-04 at 25°C) is titrated with 0.500 M NaOH. Determine the pH at the following volumes of NaOH: Volume NaOH = 20.00mL pH = 4.72 Volume NaOH = 22.50mL pH = Volume NaOH = 30.00mL pH = 12.92
A 15.00 ml aliquot of a 0.75 M solution of a weak acid (Ka = 1.50E-04 at 25°C) is titrated with 0.500 M NaOH. Determine the pH at the following volumes of NaOH: Volume NaOH = 20.00mL pH = 4.72 Volume NaOH = 22.50mL pH = Volume NaOH = 30.00mL pH = 12.92
Chemistry
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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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The answer for volume NaOH= 22.50ml is ph= 8.651
And i cant figure it out. Pls help
![A 15.00 ml aliquot of a 0.75 M solution of a weak acid (Ka = 1.50E-04 at 25°C) is titrated with 0.500 M NaOH. Determine the pH
at the following volumes of NAOH:
Volume NaOH = 20.00ML
pH =
4.72
Volume NaOH = 22.50mL
pH =
7
Volume NaOH = 30.00mL
pH = 12.92](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4b4481cb-619f-4ef0-a6b6-04bc0d22d235%2F633108e1-c086-4c41-9a93-47fab659a98e%2Fye0m4y_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 15.00 ml aliquot of a 0.75 M solution of a weak acid (Ka = 1.50E-04 at 25°C) is titrated with 0.500 M NaOH. Determine the pH
at the following volumes of NAOH:
Volume NaOH = 20.00ML
pH =
4.72
Volume NaOH = 22.50mL
pH =
7
Volume NaOH = 30.00mL
pH = 12.92
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