EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5. Complete the ICE Table below: + Hydrolysis Equation NH4+ (aq) OH (aq) NH3(aq) + H₂O(l) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NHA] = [OH-] = Write the equilibrium expression for the base dissociation constant, K, and substitute the mathematical equation containing the variable x into the equilibrium expression. Then calculate the value of [OH-] and pH of the solution. Show your complete solution. 0 +X
EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C. At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5. Complete the ICE Table below: + Hydrolysis Equation NH4+ (aq) OH (aq) NH3(aq) + H₂O(l) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NHA] = [OH-] = Write the equilibrium expression for the base dissociation constant, K, and substitute the mathematical equation containing the variable x into the equilibrium expression. Then calculate the value of [OH-] and pH of the solution. Show your complete solution. 0 +X
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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![EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C.
At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5.
Complete the ICE Table below:
+
NH4+ (aq)
OH-(aq)
Hydrolysis Equation
NH3(aq) + H₂O(l)
INITIAL
0.50
0
(Analytical molarity)
CHANGE
-X
+X
EQUILIBRIUM
(6 pts)
[NH3]
[NH4*]
=
[OH-] =
Write the equilibrium expression for the base dissociation constant, K, and substitute the
mathematical equation containing the variable x into the equilibrium expression.
Then calculate the value of [OH-] and pH of the solution. Show your complete solution.
0
+X](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb927ba68-210e-4ec1-92c1-d2ba65de5a8e%2F27ad1afa-a6b8-44fc-afeb-ee9f2d703b43%2Fw5rqq8d_processed.png&w=3840&q=75)
Transcribed Image Text:EXERCISE 2: Calculate the pH of a 0.50 M NH3 at 25°C.
At 25°C, the base dissociation constant (Kb) of ammonia (NH3 ) is 1.8 × 10-5.
Complete the ICE Table below:
+
NH4+ (aq)
OH-(aq)
Hydrolysis Equation
NH3(aq) + H₂O(l)
INITIAL
0.50
0
(Analytical molarity)
CHANGE
-X
+X
EQUILIBRIUM
(6 pts)
[NH3]
[NH4*]
=
[OH-] =
Write the equilibrium expression for the base dissociation constant, K, and substitute the
mathematical equation containing the variable x into the equilibrium expression.
Then calculate the value of [OH-] and pH of the solution. Show your complete solution.
0
+X
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