4 Consider the titration of 60.0 mt of 0.0400 M CHAN (a weak base; K 1.70e-09) with 0.100 M HBr. Calculate the pH after the following volumes of titrant have been added(a) 0.0 ml(b) 6.0 ml(c) 12.0 mLPH =8.62pH =883pH =8.73(d) 18.0 ml(0) 24.0 ml() 31.2 mlpH = 856PH = 346pH = 210Calculate the pH at the equivalence point in titrating 0.022 M solutions of each of the following with 0.078 M NaOH.(a) nitric acid (HNO3)pH =(b) phenol (HC6H5O), K = 1.3e-10pH =(c) hydrazoic acid (HN3), Ka = 1.9e-05pH =

When the volume of HBr solution is added, is lower than volume required to achieve equivalence…

Consider the titration of 60.0 mt of 0.0400 M CHN (a weak base K170e-09) with 0.100 M HBr. Calculate the pH after the following volumes of titrant have been added (a) 0.0 ml (b) 6.0 ml (c) 12.0 mL PH =8.62 PH =8.83 pH =8.73

Consider the titration of 60.0 mt of 0.0400 M CHN (a weak base K170e-09) with 0.100 M HBr. Calculate the pH after the following volumes of titrant have been added (a) 0.0 ml (b) 6.0 ml (c) 12.0 mL PH =8.62 PH =8.83 pH =8.73

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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Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

Consider the titration of 60.0 mt of 0.0400 M CHAN (a weak base; K 1.70e-09) with 0.100 M HBr. Calculate the pH after the following volumes of titrant have been added
(a) 0.0 ml
(b) 6.0 ml
(c) 12.0 mL
PH =8.62
pH =883
pH =8.73
(d) 18.0 ml
(0) 24.0 ml
() 31.2 ml
pH = 856
PH = 346
pH = 210
Calculate the pH at the equivalence point in titrating 0.022 M solutions of each of the following with 0.078 M NaOH.
(a) nitric acid (HNO3)
pH =
(b) phenol (HC6H5O), K = 1.3e-10
pH =
(c) hydrazoic acid (HN3), Ka = 1.9e-05
pH =

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