GENERAL CHEMISTRY WORKSHOP ACIDS AND BASES - 2 1. Calculate [H;O*] and [CH3COO] in an aqueous solution that is 0.100 M in both CH.COOH and CH3COONA. For acetic acid Ka = 1.8 × 10-5. 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH,)2SO4. a) What is the pH of this solution? b) If 0.88 g NaOH is added to the solution, what will be the pH? 3. You are given 250.0 mL of 0.100 M CH3CH2COOH (propionic acid, Ka = 1.35 × 105). You wish to adjust the pH by adding an appropriate solution. What volume would you add of a) no. 1.00 M HCl to lower the pH to 1.00; b) 1.00 M CH3CH2COONA to raise the pH to 4.00? 4. What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M CH3CH2COOH with 0.100 M NAOH? a) before the addition of any NaOH; b) after the addition of 10.00 mL of 0.100 M NAOH; c) after the addition of 12.50 mL of 0.100M NaOH; d) after the addition of 25.00 mL of 0.100 M NAOH; e) after the addition of 26.00 mL of 0.100 M NaOH. 5. Sodium phosphate, Na3PO4, is an ingredient of some preparations used to clean walls before they are painted. What is the pH of 1.0 M Na3PO4 (aq)? [Use Table 7.4 "Stepwise Dissociation Constants for Several Common Polyprotic Acids."] 6. a) Is an aqueous solution that is 0.10 M Na2S (aq) likely to be acidic, basic or pH neutral? Explain. b) Is an aqueous solution of ammonium cyanide, NH4CN, likely to be acidic, basic or neutral? Explain. 7. a) Calculate the pH of a 2.0 M aqueous solution of H2SO4. b) Calculate the pH of a 5.0 x 10-3 M aqueous solution of H2SO4. 8. The pH of a solution of 19.5 g of malonic acid in 0.250 L is 1.47. The pH of a 0.300 M solution of sodium hydrogen malonate is 4.26. What are the values of Kal and K2.
GENERAL CHEMISTRY WORKSHOP ACIDS AND BASES - 2 1. Calculate [H;O*] and [CH3COO] in an aqueous solution that is 0.100 M in both CH.COOH and CH3COONA. For acetic acid Ka = 1.8 × 10-5. 2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH,)2SO4. a) What is the pH of this solution? b) If 0.88 g NaOH is added to the solution, what will be the pH? 3. You are given 250.0 mL of 0.100 M CH3CH2COOH (propionic acid, Ka = 1.35 × 105). You wish to adjust the pH by adding an appropriate solution. What volume would you add of a) no. 1.00 M HCl to lower the pH to 1.00; b) 1.00 M CH3CH2COONA to raise the pH to 4.00? 4. What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M CH3CH2COOH with 0.100 M NAOH? a) before the addition of any NaOH; b) after the addition of 10.00 mL of 0.100 M NAOH; c) after the addition of 12.50 mL of 0.100M NaOH; d) after the addition of 25.00 mL of 0.100 M NAOH; e) after the addition of 26.00 mL of 0.100 M NaOH. 5. Sodium phosphate, Na3PO4, is an ingredient of some preparations used to clean walls before they are painted. What is the pH of 1.0 M Na3PO4 (aq)? [Use Table 7.4 "Stepwise Dissociation Constants for Several Common Polyprotic Acids."] 6. a) Is an aqueous solution that is 0.10 M Na2S (aq) likely to be acidic, basic or pH neutral? Explain. b) Is an aqueous solution of ammonium cyanide, NH4CN, likely to be acidic, basic or neutral? Explain. 7. a) Calculate the pH of a 2.0 M aqueous solution of H2SO4. b) Calculate the pH of a 5.0 x 10-3 M aqueous solution of H2SO4. 8. The pH of a solution of 19.5 g of malonic acid in 0.250 L is 1.47. The pH of a 0.300 M solution of sodium hydrogen malonate is 4.26. What are the values of Kal and K2.
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
![GENERAL CHEMISTRY WORKSHOP
ACIDS AND BASES - 2
1. Calculate [H;O*] and [CH3COO] in an aqueous solution that is 0.100 M in both CH.COOH
and CH3COONA. For acetic acid Ka = 1.8 × 10-5.
2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH,)2SO4. a) What is
the pH of this solution? b) If 0.88 g NaOH is added to the solution, what will be the pH?
3. You are given 250.0 mL of 0.100 M CH3CH2COOH (propionic acid, Ka = 1.35 × 105). You
wish to adjust the pH by adding an appropriate solution. What volume would you add of a)
no.
1.00 M HCl to lower the pH to 1.00; b) 1.00 M CH3CH2COONA to raise the pH to 4.00?
4. What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M
CH3CH2COOH with 0.100 M NAOH? a) before the addition of any NaOH; b) after the
addition of 10.00 mL of 0.100 M NAOH; c) after the addition of 12.50 mL of 0.100M
NaOH; d) after the addition of 25.00 mL of 0.100 M NAOH; e) after the addition of 26.00
mL of 0.100 M NaOH.
5. Sodium phosphate, Na3PO4, is an ingredient of some preparations used to clean walls before
they are painted. What is the pH of 1.0 M Na3PO4 (aq)? [Use Table 7.4 "Stepwise
Dissociation Constants for Several Common Polyprotic Acids."]
6. a) Is an aqueous solution that is 0.10 M Na2S (aq) likely to be acidic, basic or pH neutral?
Explain. b) Is an aqueous solution of ammonium cyanide, NH4CN, likely to be acidic, basic
or neutral? Explain.
7. a) Calculate the pH of a 2.0 M aqueous solution of H2SO4.
b) Calculate the pH of a 5.0 x 10-3 M aqueous solution of H2SO4.
8. The pH of a solution of 19.5 g of malonic acid in 0.250 L is 1.47. The pH of a 0.300 M
solution of sodium hydrogen malonate is 4.26. What are the values of Kal and K2.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbecc57bd-691c-44b9-b5ef-c7430b91fff8%2Fd6092390-cebe-47c4-8d90-7ee1f22e0a2e%2Fs8gflsa9.jpeg&w=3840&q=75)
Transcribed Image Text:GENERAL CHEMISTRY WORKSHOP
ACIDS AND BASES - 2
1. Calculate [H;O*] and [CH3COO] in an aqueous solution that is 0.100 M in both CH.COOH
and CH3COONA. For acetic acid Ka = 1.8 × 10-5.
2. A buffer solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH,)2SO4. a) What is
the pH of this solution? b) If 0.88 g NaOH is added to the solution, what will be the pH?
3. You are given 250.0 mL of 0.100 M CH3CH2COOH (propionic acid, Ka = 1.35 × 105). You
wish to adjust the pH by adding an appropriate solution. What volume would you add of a)
no.
1.00 M HCl to lower the pH to 1.00; b) 1.00 M CH3CH2COONA to raise the pH to 4.00?
4. What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M
CH3CH2COOH with 0.100 M NAOH? a) before the addition of any NaOH; b) after the
addition of 10.00 mL of 0.100 M NAOH; c) after the addition of 12.50 mL of 0.100M
NaOH; d) after the addition of 25.00 mL of 0.100 M NAOH; e) after the addition of 26.00
mL of 0.100 M NaOH.
5. Sodium phosphate, Na3PO4, is an ingredient of some preparations used to clean walls before
they are painted. What is the pH of 1.0 M Na3PO4 (aq)? [Use Table 7.4 "Stepwise
Dissociation Constants for Several Common Polyprotic Acids."]
6. a) Is an aqueous solution that is 0.10 M Na2S (aq) likely to be acidic, basic or pH neutral?
Explain. b) Is an aqueous solution of ammonium cyanide, NH4CN, likely to be acidic, basic
or neutral? Explain.
7. a) Calculate the pH of a 2.0 M aqueous solution of H2SO4.
b) Calculate the pH of a 5.0 x 10-3 M aqueous solution of H2SO4.
8. The pH of a solution of 19.5 g of malonic acid in 0.250 L is 1.47. The pH of a 0.300 M
solution of sodium hydrogen malonate is 4.26. What are the values of Kal and K2.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY