Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL pH = b. 10.0 mL pH = c. 50.0 mL pH = d. 80.0 mL pH = e. 120.0 mL pH =
Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL pH = b. 10.0 mL pH = c. 50.0 mL pH = d. 80.0 mL pH = e. 120.0 mL pH =
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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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:Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M
KOH. Calculate the pH of the resulting solution after the following
volumes of KOH have been added.
a. 0.0 mL
pH =
b. 10.0 mL
pH =
c. 50.0 mL
pH =
d. 80.0 mL
pH =
e. 120.0 mL
pH =
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Step 1: Analysis of the nature of acid and base
VIEWStep 2: Formulas for hydrogen ion and hydroxide ion concentration
VIEWStep 3: pH at the start
VIEWStep 4: pH on addition of 10.0mL KOH
VIEWStep 5: pH on addition of 50mL KOH
VIEWStep 6: On addition of 80mL KOH
VIEWStep 7: On addition of 120mL KOH
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