A. Calculate the pH of 35.00 mL of acetic acid using the concentration assigned in Beyond Labz: HC,H;O, (aa) 2H* (aa) +C,H;O; (aa) I Initial Concentration (M) 0.1031 Change in Concentration (M) -x +x +x Equilibrium Concentration (M) 0.1031 - x E Equilibrium Concentration, Calculated (M) 1. Initial concentration [HC,H;O,]o = 0.1031 M 2. K, symbolic expression: [H* ][ C,H;O; ] [HC,H;O3] (x)(x) 3. K, numerical equation with x: 1.8x 105 = 0.1031 -x 4. Quadratic Formula Method a. Quadratic equation: b.Quadratic formula:| 5. Assumption (5% rule) Method a.Equation for x: b.% ionization = 6. Equilibrium concentrations a [HC,H;Ola = b.[H*la = c.[C,H;O; ha = 7. pH =
A. Calculate the pH of 35.00 mL of acetic acid using the concentration assigned in Beyond Labz: HC,H;O, (aa) 2H* (aa) +C,H;O; (aa) I Initial Concentration (M) 0.1031 Change in Concentration (M) -x +x +x Equilibrium Concentration (M) 0.1031 - x E Equilibrium Concentration, Calculated (M) 1. Initial concentration [HC,H;O,]o = 0.1031 M 2. K, symbolic expression: [H* ][ C,H;O; ] [HC,H;O3] (x)(x) 3. K, numerical equation with x: 1.8x 105 = 0.1031 -x 4. Quadratic Formula Method a. Quadratic equation: b.Quadratic formula:| 5. Assumption (5% rule) Method a.Equation for x: b.% ionization = 6. Equilibrium concentrations a [HC,H;Ola = b.[H*la = c.[C,H;O; ha = 7. pH =
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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Need to Solve e and 4,5,6,7
![A. Calculate the pH of 35.00 mL of acetic acid using the concentration assigned in Beyond Labz:
HC,H;O, (aa)
2H* (aa)
+C,H;O; (aa)
I
Initial Concentration (M) 0.1031
Change in Concentration (M) -x
+x
+x
Equilibrium Concentration (M) 0.1031 - x
E
Equilibrium Concentration,
Calculated (M)
1. Initial concentration [HC,H;O,]o = 0.1031 M
2. K, symbolic expression: [H* ][ C,H;O; ]
[HC,H;O3]
(x)(x)
3. K, numerical equation with x: 1.8x 105 =
0.1031 -x
4. Quadratic Formula Method
a. Quadratic equation:
b.Quadratic formula:|
5. Assumption (5% rule) Method
a.Equation for x:
b.% ionization =
6. Equilibrium concentrations
a [HC,H;Ola =
b.[H*la =
c.[C,H;O; ha =
7. pH =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f55c28e-71db-47ea-b0ac-f3ad1a1e82a5%2F689c0c94-1b60-4705-86cf-03d7a638f4ea%2Fjzzqme_processed.png&w=3840&q=75)
Transcribed Image Text:A. Calculate the pH of 35.00 mL of acetic acid using the concentration assigned in Beyond Labz:
HC,H;O, (aa)
2H* (aa)
+C,H;O; (aa)
I
Initial Concentration (M) 0.1031
Change in Concentration (M) -x
+x
+x
Equilibrium Concentration (M) 0.1031 - x
E
Equilibrium Concentration,
Calculated (M)
1. Initial concentration [HC,H;O,]o = 0.1031 M
2. K, symbolic expression: [H* ][ C,H;O; ]
[HC,H;O3]
(x)(x)
3. K, numerical equation with x: 1.8x 105 =
0.1031 -x
4. Quadratic Formula Method
a. Quadratic equation:
b.Quadratic formula:|
5. Assumption (5% rule) Method
a.Equation for x:
b.% ionization =
6. Equilibrium concentrations
a [HC,H;Ola =
b.[H*la =
c.[C,H;O; ha =
7. pH =
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