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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
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
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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
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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