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: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 77QAP: Two students were asked to determine the Kb of an unknown base. They were given a bottle with a...
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![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.
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