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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Theory
In the previous lab, the dissolution of potassium bitartrate was described by the following
chemical equation:
KHC4H4O6(s) K(aq) + HC4H4O6 (aq)
To simplify notation, potassium bitartrate (KHC4H4O6) was denoted as KHT and the
bitartrate ion (HC4H406) will be denoted as HT where the H denotes an acidic proton:
KHT(s) K (aq) + HT (aq)
The solubility product constant for this process can be written as:
(1)
To determine the Ksp for this reaction, the equilibrium concentrations for K* and HT must be
measured in a saturated solution of KHT. When enough solid KHT is added to pure water so
that a saturated solution of KHT is prepared, then [K*]eq = [HT]eq. This leads to a
simplification of eq. 1, Ksp = [HT]eq². The equilibrium concentration of HT is readily
determined by titrating the solution with OH:
[HT ] eq
Ksp [K]eq[HT]eq
=
moles of HT-
volume of HT-at beginning of titration
(2)
The equivalence point for the titration is determined using phenolphthalein as an indicator.
Since KHT has been dissolved in pure water, the [HT-lea also represents the molar solubility
of KHT (i.e. how many moles of KHT will dissolve in one liter of water). The Gibbs Free
Energy change can be readily calculated from:
AG = -RT In(Ksp)
The equilibrium constant depends upon temperature and it can be shown that
(3)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd63ec96b-7fd4-4095-9c7d-e9d8aa5316e9%2F3fcfb381-93f2-4ee0-ac4e-37150da30fb1%2Fua10jjf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1 of 3
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Theory
In the previous lab, the dissolution of potassium bitartrate was described by the following
chemical equation:
KHC4H4O6(s) K(aq) + HC4H4O6 (aq)
To simplify notation, potassium bitartrate (KHC4H4O6) was denoted as KHT and the
bitartrate ion (HC4H406) will be denoted as HT where the H denotes an acidic proton:
KHT(s) K (aq) + HT (aq)
The solubility product constant for this process can be written as:
(1)
To determine the Ksp for this reaction, the equilibrium concentrations for K* and HT must be
measured in a saturated solution of KHT. When enough solid KHT is added to pure water so
that a saturated solution of KHT is prepared, then [K*]eq = [HT]eq. This leads to a
simplification of eq. 1, Ksp = [HT]eq². The equilibrium concentration of HT is readily
determined by titrating the solution with OH:
[HT ] eq
Ksp [K]eq[HT]eq
=
moles of HT-
volume of HT-at beginning of titration
(2)
The equivalence point for the titration is determined using phenolphthalein as an indicator.
Since KHT has been dissolved in pure water, the [HT-lea also represents the molar solubility
of KHT (i.e. how many moles of KHT will dissolve in one liter of water). The Gibbs Free
Energy change can be readily calculated from:
AG = -RT In(Ksp)
The equilibrium constant depends upon temperature and it can be shown that
(3)
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1. Write the chemical reaction for the titration of the filtered KHT solution with NaOH.
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