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 x 10-5. Step 1. Complete the ICE Table below: Hydrolysis Equation NH3(aq) + H₂O(l) NH, (aq) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NH] = [OH] = Step 2. Write the equilibrium expression for the base dissociation constant, Kt Kb = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the value of [OH]. Show the complete solution. SOLUTION Step 5. Calculate pH of the solution. Show the complete solution. Answer: + OH (aq) 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 x 10-5. Step 1. Complete the ICE Table below: Hydrolysis Equation NH3(aq) + H₂O(l) NH, (aq) INITIAL 0.50 0 (Analytical molarity) CHANGE -X +X EQUILIBRIUM (6 pts) [NH3] = [NH] = [OH] = Step 2. Write the equilibrium expression for the base dissociation constant, Kt Kb = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the value of [OH]. Show the complete solution. SOLUTION Step 5. Calculate pH of the solution. Show the complete solution. Answer: + OH (aq) 0 +X
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section16.6: Buffers
Problem 16.6CC: The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base,...
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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 x 10-5.
Step 1. Complete the ICE Table below:
Hydrolysis Equation
NH, (aq)
NH3(aq) + H₂O(l)
INITIAL
0.50
0
(Analytical molarity)
CHANGE
-X
+X
EQUILIBRIUM
(6 pts)
[NH3]
=
[NH₂¹] =
[OH] =
Step 2. Write the equilibrium expression for the base dissociation constant, Kt
Kb =
Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression.
Answer:
Step 4 Calculate the value of [OH]. Show the complete solution.
SOLUTION
Step 5. Calculate pH of the solution. Show the complete solution. (
Answer:
+
OH (aq)
0
+X](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe6632444-f30b-4f54-8e4a-3ffbb89bd0c3%2F5c2d2c6d-a9ed-4890-99d2-850d3571d7ef%2Fwdo3eug_processed.jpeg&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 x 10-5.
Step 1. Complete the ICE Table below:
Hydrolysis Equation
NH, (aq)
NH3(aq) + H₂O(l)
INITIAL
0.50
0
(Analytical molarity)
CHANGE
-X
+X
EQUILIBRIUM
(6 pts)
[NH3]
=
[NH₂¹] =
[OH] =
Step 2. Write the equilibrium expression for the base dissociation constant, Kt
Kb =
Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression.
Answer:
Step 4 Calculate the value of [OH]. Show the complete solution.
SOLUTION
Step 5. Calculate pH of the solution. Show the complete solution. (
Answer:
+
OH (aq)
0
+X
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