Consider the reaction of a 20.0 mL of 0.220 M CsHsNHCI (Ka = 5.9 x 10-) with 12.0 mL of 0.215 M CSOH. a) Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction. b) What quantity in moles of CsHsNH+ would be present at the start of the titration? c) What quantity in moles of OH- would be present if 12.0 mL of OH- were added?

Consider the reaction of a 20.0 mL of 0.220 M CsHsNHCI (Ka = 5.9 x 10-) with 12.0 mL of 0.215 M CSOH. a) Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction. b) What quantity in moles of CsHsNH+ would be present at the start of the titration? c) What quantity in moles of OH- would be present if 12.0 mL of OH- were added?

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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Question

Consider the reaction of a 20.0 mL of 0.220 M CsH5NHCI (Ka = 5.9 x
10-6) with 12.0 mL of 0.215 M CSOH.
a) Write the net ionic equation for the reaction that takes place. Be sure to
include the proper phases for all species within the reaction.
b) What quantity in moles of CsHsNH+ would be present at the start of the
titration?
c) What quantity in moles of OH- would be present if 12.0 mL of OH- were
added?
d) What species would be left in the beaker after the reaction goes to
completion?

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