Part (c) and (d) only Short Answer Section1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NaOH. The results of this titrationis shown below.1412a.10Referring to a chart of indicators andtheir turning points, which indicatorwould you use for this titration?Explain.8F6The4Suitable indicator for the titration.weak and and strong base NaOH (₂)either thymol blue (pt lange 8.k9.6) or phenolphta lein (pH range 6.3-10.0).020would be5070403060Volume of NaOH addod (ml)b. Using the symbol "HA" to represent the weak acid, use a dissociation equation to explainwhy this acid behaves as a weak acidA jaqlThe dissociation of a weak acid HAWhere the equilibriuma strong basecan be depicted as . Hacaq) = H (4₂) +is very weak,lies more to the left dissociationand highly unstable. So, equilibrium lies to the left.c. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change verymuch. How does Le Chatelier's Principle explain this phenomenon?d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful toset up an ICE table as part ofyour solution!1080

The resistance in the change in pH of the solution during the buffer range is needed to be explained…

C. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change very much. How does Le Chatelier's Principle explain this phenomenon? d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful to set up an ICE table as part of your solution

C. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change very much. How does Le Chatelier's Principle explain this phenomenon? d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful to set up an ICE table as part of your solution

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 99AP

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

100%

Part (c) and (d) only

Short Answer Section
1. 10.0 mL of 0.40 M weak acid is being neutralized with 0.10 M NaOH. The results of this titration
is shown below.
14
12
a.
10
Referring to a chart of indicators and
their turning points, which indicator
would you use for this titration?
Explain.
8
F
6
The
4
Suitable indicator for the titration.
weak and and strong base NaOH (₂)
either thymol blue (pt lange 8.k
9.6) or phenolphta lein (pH range 6.3-10.0).
0
20
would be
50
70
40
30
60
Volume of NaOH addod (ml)
b. Using the symbol "HA" to represent the weak acid, use a dissociation equation to explain
why this acid behaves as a weak acid
A jaql
The dissociation of a weak acid HA
Where the equilibrium
a strong base
can be depicted as . Hacaq) = H (4₂) +
is very weak,
lies more to the left dissociation
and highly unstable. So, equilibrium lies to the left.
c. In the buffer zone between 20 and 30 mL of titrant added the pH doesn't change very
much. How does Le Chatelier's Principle explain this phenomenon?
d. Using the pH at the start of the titration, find the K, for this acid. You may find it helpful to
set up an ICE table as part of
your solution!
10
80

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