2020Consider the reaction of a 20.0 mL of 0.220 M CsHsNHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.231 MCsOH.abLWrite the net ionic equation for the reaction that takes place. Be sure to includethe proper phases for all species within the reaction.What quantity in moles of CsHsNH+ would be present at the start of the titration?CLWhat quantity in moles of OH- would be present in 12.0 mL of CSOH solution?P(DefgLWhat species would be left in the beaker after the reaction goes to completion?What quantity in moles of CsHsNH+ would be left in the beaker after the reaction goes tocompletion?L What quantity in moles of CsHsN are produced after the reaction goes to completion?LWhat would be the pH of this solution after the reaction goes to completion and thesystem reaches equilibrium?

Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

20 a Consider the reaction of a 20.0 mL of 0.220 M CsHsNHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.231 M CsOH. 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 d e L What quantity in moles of OH- would be present in 12.0 mL of CSOH solution? L What species would be left in the beaker after the reaction goes to completion? L What quantity in moles of CsHsNH* would be left in the beaker after the reaction goes to completion? f L What quantity in moles of CsH&N are produced after the reaction goes to completion? L What would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium?

20 a Consider the reaction of a 20.0 mL of 0.220 M CsHsNHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.231 M CsOH. 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 d e L What quantity in moles of OH- would be present in 12.0 mL of CSOH solution? L What species would be left in the beaker after the reaction goes to completion? L What quantity in moles of CsHsNH* would be left in the beaker after the reaction goes to completion? f L What quantity in moles of CsH&N are produced after the reaction goes to completion? L What would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium?

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

20
20
Consider the reaction of a 20.0 mL of 0.220 M CsHsNHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.231 M
CsOH.
a
b
L
Write the net ionic equation for the reaction that takes place. Be sure to include
the proper phases for all species within the reaction.
What quantity in moles of CsHsNH+ would be present at the start of the titration?
C
L
What quantity in moles of OH- would be present in 12.0 mL of CSOH solution?
P
(D
e
f
g
L
What species would be left in the beaker after the reaction goes to completion?
What quantity in moles of CsHsNH+ would be left in the beaker after the reaction goes to
completion?
L What quantity in moles of CsHsN are produced after the reaction goes to completion?
L
What would be the pH of this solution after the reaction goes to completion and the
system reaches equilibrium?

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