1. Write the dissociation equation in water and equilibrium constant expression for the dissociation of the following weak acid. a. Hypochlorous acid, HOCI Ka = 3.0 x 10-8 b. propionic acid, CH3CH2COOH Ka 1.35 x 10-5 %3D 2. Write the dissociation equation and equilibrium constant expression for the dissociation of the following weak bases a. Methylamine, CH3NH2, Kb = 3.5 x 104 %3D b. formate ion, COOH Kb = 5.5 x 10-11 3. Calculate the [H3O*], [OH'], pH and pOH of a 0.120 M HNO2 (nitrous acid). Ка 3D7.10 х 10-4 4. Calculate the [OH], [H3O*], pOH and pH of a 0.0750 M NH3 Ka NH4* = 5.70x 10 -10 5. Calculate the pH and [H3O*] of a buffer solution prepared by dissolving 0.218 mol of NaC2H3O2 in 500.mL of 100 М НC2Н3О2. Kа HC2H302 %3D 1.80 х 105
1. Write the dissociation equation in water and equilibrium constant expression for the dissociation of the following weak acid. a. Hypochlorous acid, HOCI Ka = 3.0 x 10-8 b. propionic acid, CH3CH2COOH Ka 1.35 x 10-5 %3D 2. Write the dissociation equation and equilibrium constant expression for the dissociation of the following weak bases a. Methylamine, CH3NH2, Kb = 3.5 x 104 %3D b. formate ion, COOH Kb = 5.5 x 10-11 3. Calculate the [H3O*], [OH'], pH and pOH of a 0.120 M HNO2 (nitrous acid). Ка 3D7.10 х 10-4 4. Calculate the [OH], [H3O*], pOH and pH of a 0.0750 M NH3 Ka NH4* = 5.70x 10 -10 5. Calculate the pH and [H3O*] of a buffer solution prepared by dissolving 0.218 mol of NaC2H3O2 in 500.mL of 100 М НC2Н3О2. Kа HC2H302 %3D 1.80 х 105
Chemistry
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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
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![1. Write the dissociation equation in water and equilibrium constant expression for the dissociation
of the following weak acid.
a. Hypochlorous acid, HOCI
Ka = 3.0 x 10-8
b. propionic acid, CH3CH2COOH Ka
1.35 x 10-5
%3D
2. Write the dissociation equation and equilibrium constant expression for the dissociation of the
following weak bases
a. Methylamine, CH3NH2, Kb = 3.5 x 104
%3D
b. formate ion, COOH Kb = 5.5 x 10-11
3. Calculate the [H3O*], [OH'], pH and pOH of a 0.120 M HNO2 (nitrous acid).
Ка 3D7.10 х 10-4
4. Calculate the [OH], [H3O*], pOH and pH of a 0.0750 M NH3
Ka NH4* = 5.70x 10
-10
5. Calculate the pH and [H3O*] of a buffer solution prepared by dissolving 0.218 mol of NaC2H3O2
in 500.mL of 100 М НC2Н3О2. Kа HC2H302 %3D 1.80 х 105](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fba952051-6232-4dba-80c0-7865e27d383a%2F9f4811af-e2a0-4b80-b4a2-1f9be1069804%2Fh1neda.jpeg&w=3840&q=75)
Transcribed Image Text:1. Write the dissociation equation in water and equilibrium constant expression for the dissociation
of the following weak acid.
a. Hypochlorous acid, HOCI
Ka = 3.0 x 10-8
b. propionic acid, CH3CH2COOH Ka
1.35 x 10-5
%3D
2. Write the dissociation equation and equilibrium constant expression for the dissociation of the
following weak bases
a. Methylamine, CH3NH2, Kb = 3.5 x 104
%3D
b. formate ion, COOH Kb = 5.5 x 10-11
3. Calculate the [H3O*], [OH'], pH and pOH of a 0.120 M HNO2 (nitrous acid).
Ка 3D7.10 х 10-4
4. Calculate the [OH], [H3O*], pOH and pH of a 0.0750 M NH3
Ka NH4* = 5.70x 10
-10
5. Calculate the pH and [H3O*] of a buffer solution prepared by dissolving 0.218 mol of NaC2H3O2
in 500.mL of 100 М НC2Н3О2. Kа HC2H302 %3D 1.80 х 105
![](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fba952051-6232-4dba-80c0-7865e27d383a%2F9f4811af-e2a0-4b80-b4a2-1f9be1069804%2Fp1zojn.jpeg&w=3840&q=75)
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