B. Determination of the hydrolysis constant (or acid dissociation constant,Ka) of NH4+.1. Consider a 0.01 M NH4CI solution.2. Write the dissociation equation for NH4CI.3. Identify the ion/s that can undergo hydrolysis.4. It has been determined experimentally that the pH of 0.01 M NH4CI solution is5.91. From the pH of the solution, solve for the concentration of all speciespresent in the solution. Input all your answers in Tables 2 and 3.5. Solve for the Ka of NH4+.6. Compare your experimental value to the literature value for the Ka of NH4+.B. Determination of the hydrolysis constant (or acid dissociation constant,Ka) of NH4*.Table 2. Dissociation of NH,CIDissociation equation of NH4CIpH of solutionlon that undergoes hydrolysis:Hydrolysis reactionTable 3. ICE Table for the Hydrolysis of NH4*Parameter[NH,*][H*][NH3]Initial concentrationChange inconcentrationEquilibriumConcentrationSolving for the hydrolysis constant, Kn (or Ka) of NH4+Theoretical Value for Ka of NH4+% Error:

Given: Concentration of NH4Cl =0.01 M pH of the solution: 5.91 To determine: Hydrolysis constant of…

Answered: B. Determination of the hydrolysis…

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B. Determination of the hydrolysis constant (or acid dissociation constant, Ka) of NH4+.

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

B. Determination of the hydrolysis constant (or acid dissociation constant,
Ka) of NH4+.
1. Consider a 0.01 M NH4CI solution.
2. Write the dissociation equation for NH4CI.
3. Identify the ion/s that can undergo hydrolysis.
4. It has been determined experimentally that the pH of 0.01 M NH4CI solution is
5.91. From the pH of the solution, solve for the concentration of all species
present in the solution. Input all your answers in Tables 2 and 3.
5. Solve for the Ka of NH4+.
6. Compare your experimental value to the literature value for the Ka of NH4+.
B. Determination of the hydrolysis constant (or acid dissociation constant,
Ka) of NH4*.
Table 2. Dissociation of NH,CI
Dissociation equation of NH4CI
pH of solution
lon that undergoes hydrolysis:
Hydrolysis reaction
Table 3. ICE Table for the Hydrolysis of NH4*
Parameter
[NH,*]
[H*]
[NH3]
Initial concentration
Change in
concentration
Equilibrium
Concentration
Solving for the hydrolysis constant, Kn (or Ka) of NH4+
Theoretical Value for Ka of NH4+
% Error:

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