EXERCISE 1: Calculate the pH of a 0.50 M HA at 25°C. At 25°C, the acid dissociation constant (K₂) of the monoprotic weak acid, HA, is 7.2 x 10-6. Step 1. Complete the ICE Table below: Dissociation Equation H+ (aq) A-(aq) INITIAL 0 Concentration CHANGE +X EQUILIBRIUM Concentration [HA] = [H+] = [A-] = Step 2. Write the equilibrium expression for the acid dissociation constant, Ka. K₂ = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the [H+]. Show the complete solution. Answer: Step 5. Calculate pH of the solution. Show the complete solution. Answer: HA(aq) 0.500 -X 0 +X
EXERCISE 1: Calculate the pH of a 0.50 M HA at 25°C. At 25°C, the acid dissociation constant (K₂) of the monoprotic weak acid, HA, is 7.2 x 10-6. Step 1. Complete the ICE Table below: Dissociation Equation H+ (aq) A-(aq) INITIAL 0 Concentration CHANGE +X EQUILIBRIUM Concentration [HA] = [H+] = [A-] = Step 2. Write the equilibrium expression for the acid dissociation constant, Ka. K₂ = Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression. Answer: Step 4 Calculate the [H+]. Show the complete solution. Answer: Step 5. Calculate pH of the solution. Show the complete solution. Answer: HA(aq) 0.500 -X 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 1: Calculate the pH of a 0.50 M HA at 25°C.
At 25°C, the acid dissociation constant (K₂) of the monoprotic weak acid, HA, is 7.2 x 10-6.
Step 1. Complete the ICE Table below:
Dissociation Equation
H+ (aq)
A-(aq)
INITIAL
0
Concentration
CHANGE
+X
EQUILIBRIUM
Concentration
[HA] =
[H+] =
[A-] =
Step 2. Write the equilibrium expression for the acid dissociation constant, Ka.
Ka =
Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression.
Answer:
Step 4 Calculate the [H+]. Show the complete solution.
Answer:
Step 5. Calculate pH of the solution. Show the complete solution.
Answer:
HA(aq)
0.500
-X
0
+X](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60242f42-493f-4bd0-82bb-acea33cb80f8%2Fe861962a-24f4-4cfe-a02d-0e691799dfc7%2F17qg95_processed.png&w=3840&q=75)
Transcribed Image Text:EXERCISE 1: Calculate the pH of a 0.50 M HA at 25°C.
At 25°C, the acid dissociation constant (K₂) of the monoprotic weak acid, HA, is 7.2 x 10-6.
Step 1. Complete the ICE Table below:
Dissociation Equation
H+ (aq)
A-(aq)
INITIAL
0
Concentration
CHANGE
+X
EQUILIBRIUM
Concentration
[HA] =
[H+] =
[A-] =
Step 2. Write the equilibrium expression for the acid dissociation constant, Ka.
Ka =
Step 3. Substitute the mathematical equation containing the variable x into the equilibrium expression.
Answer:
Step 4 Calculate the [H+]. Show the complete solution.
Answer:
Step 5. Calculate pH of the solution. Show the complete solution.
Answer:
HA(aq)
0.500
-X
0
+X
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