Solve the folowing problems. 1. Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONA. 2. What is the pH of the buffer system after the addition of 0.10 mole of gaseous HCI toIL of the solution. Frame: 10 minutes)
Solve the folowing problems. 1. Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONA. 2. What is the pH of the buffer system after the addition of 0.10 mole of gaseous HCI toIL of the solution. Frame: 10 minutes)
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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Hi! Can someone answer learning task 4, no. 2? Thanks!
![[CH3COOH] = 0.20 M [CH3COONA] = 0.30 M
Ka= [H*l[CH3COOH1.
[CH3COOH]
[H*] = Ka[CH3COOH] = [1,8 x10-5)[ 0.20)= 1.2 x105 M
%3D
[CH3COOH]
0.30
pH= -log [H*]
3 -log (1.2 x10-5)
= 4.92
%3D
%3D
Solve for pka = -log Ka = 4og (1.8 x10-5) = 4.74
%3D
To calculate for the pH of the solution
pH = pH3pKa + log ICH3COOH-1 = 4.74 + log 0.30 M = 4.74 + 0.18 = 4.92
%3D
%3D
%3D
[CH3COOH]
0.20 M
E. Engagement (Time Frame: 3 hours)
Learning Task 2
Solve the folowing problems.
1. The concentration of H* ions in a bottle of table wine was 3.2 x 10 M right after the cork was removed. Only half of
the wine was consumed. The other half, after it had been standing open to the air for a month, was found to have a H* ion
concentration equal to 1.0 x 103 M. Calculate the pH of the wine on each of these occasions.
2. The pH of rainwater collected in ANHS on a parficular day was 4.82. Calculate the H ion concentration of the
rainwater.
3. Find the pH if the [OH] is equal to 1.0 x 10 M.
Learning Task 3
Identify the buffer systems below:
1. KH2PO4/ H3PO4
2. NaCIO4 /HCIO4
3. KF /HF
4. KBr /HBr
5. Na2CO3/NaHCO3
Learning Task 4
Solve the folowing problems.
1. Calculate the pH of a buffer system containing 1.0M CH3COOH and 1.0 M CH3COONA.
2. What is the pH of the buffer system after the addition of 0.10 mole of gaseous HCI to 1 L of the solution.
A. Assimilation (Time Frame: 10 minutes)
remains after one proton has been extracted from the acid. A conjugate acid, on the other hand, is formed when a proton
in dofined as the negative of the logarithm of the hydrogen
Bronsted acids donate protons and Bronsted bases accept protons. A Bronsted acid's conjugate base is the species that
d base](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2f458cbc-20dd-4435-b41b-56e298bd15db%2F70e3a121-c600-4f0c-b761-251837fbf576%2Fhnny66a_processed.jpeg&w=3840&q=75)
Transcribed Image Text:[CH3COOH] = 0.20 M [CH3COONA] = 0.30 M
Ka= [H*l[CH3COOH1.
[CH3COOH]
[H*] = Ka[CH3COOH] = [1,8 x10-5)[ 0.20)= 1.2 x105 M
%3D
[CH3COOH]
0.30
pH= -log [H*]
3 -log (1.2 x10-5)
= 4.92
%3D
%3D
Solve for pka = -log Ka = 4og (1.8 x10-5) = 4.74
%3D
To calculate for the pH of the solution
pH = pH3pKa + log ICH3COOH-1 = 4.74 + log 0.30 M = 4.74 + 0.18 = 4.92
%3D
%3D
%3D
[CH3COOH]
0.20 M
E. Engagement (Time Frame: 3 hours)
Learning Task 2
Solve the folowing problems.
1. The concentration of H* ions in a bottle of table wine was 3.2 x 10 M right after the cork was removed. Only half of
the wine was consumed. The other half, after it had been standing open to the air for a month, was found to have a H* ion
concentration equal to 1.0 x 103 M. Calculate the pH of the wine on each of these occasions.
2. The pH of rainwater collected in ANHS on a parficular day was 4.82. Calculate the H ion concentration of the
rainwater.
3. Find the pH if the [OH] is equal to 1.0 x 10 M.
Learning Task 3
Identify the buffer systems below:
1. KH2PO4/ H3PO4
2. NaCIO4 /HCIO4
3. KF /HF
4. KBr /HBr
5. Na2CO3/NaHCO3
Learning Task 4
Solve the folowing problems.
1. Calculate the pH of a buffer system containing 1.0M CH3COOH and 1.0 M CH3COONA.
2. What is the pH of the buffer system after the addition of 0.10 mole of gaseous HCI to 1 L of the solution.
A. Assimilation (Time Frame: 10 minutes)
remains after one proton has been extracted from the acid. A conjugate acid, on the other hand, is formed when a proton
in dofined as the negative of the logarithm of the hydrogen
Bronsted acids donate protons and Bronsted bases accept protons. A Bronsted acid's conjugate base is the species that
d base
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