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...
Related questions
Question
Hi! Can someone answer learning task 3? Kindly provide an explanation. Thank you!
![[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%2F2d523921-adf9-45bd-ac14-ad9079dca907%2Few4trja_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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