For the following table of potentiometric titration of weak acid (10 mL) vs strong base (0.1 M) 1. Draw the titration curve 2. Draw the 1st derivative titration curve 3. Calculate: a) eq. point b) pka of the acid c) Ka of the acid V (mL) pH 2.7 1 2.8 2 3 4 3.3 3.4 3.7 6.1 3.8 6.2 3.9 6.3 4 6.4 4.1 6.5 4.9 6.6 5.7 6.7 5.9 6.8 6.9 6.2 7 6.4 8 6.7 7.1 10 7.2 11 7.3 12 7.4 13 7.5 14 7.6 15 7.6

For the following table of potentiometric titration of weak acid (10 mL) vs strong base (0.1 M) 1. Draw the titration curve 2. Draw the 1st derivative titration curve 3. Calculate: a) eq. point b) pka of the acid c) Ka of the acid V (mL) pH 2.7 1 2.8 2 3 4 3.3 3.4 3.7 6.1 3.8 6.2 3.9 6.3 4 6.4 4.1 6.5 4.9 6.6 5.7 6.7 5.9 6.8 6.9 6.2 7 6.4 8 6.7 7.1 10 7.2 11 7.3 12 7.4 13 7.5 14 7.6 15 7.6

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 16.53QE

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Determination of K, TRIAL Volume NaOH at pH at Midpoint of Titration Midpoint of Titration 1. 3.22 3. Average K Identity of Unknown Acid
17.6
BURETTE READING SAMPLE Pp Mo A 12.4 25.0 6.2 6.2 9.2 16.8 D. 0.0 5.3 Use the table below to identify the basic compound C: *Note that double indicator titration for each compound was done using a standard acid solution with 0.0 mL as initial reading. O NaHCO3 O NaOHANazCO3 O NaOHANaHCO3 O Nazco3