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8. Which of the following combinations would act as buffered solutions (look at the ions individually)? JUSTIFY why. a. HCI and NaCl b. CH3COOH and KCH³COO c. H₂S and NaHS

8. Which of the following combinations would act as buffered solutions (look at the ions individually)? JUSTIFY why. a. HCI and NaCl b. CH3COOH and KCH³COO c. H₂S and NaHS

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
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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Please help with question 8
Topic 14 HW 4. In each of the following chemical equations, identify the conjugate acid-base pairs. a. CH3NH2 + H₂O CH3NH3+ + OH- 5. Write a chemical equation showing how each of the following species can behave as indicated when dissolved in water(this is the other reactant). a. HSO3 as an acid A B 6. Complete the following table. Show all calculations in the open space, clearly labeled. Solution pH POH [H+] [OH-] PUO b. CH3COOH + NH3 CH3COO- + NH4+ C b. CO32- as a base D 9.63 1.22 3.9x10-6M 7. Solution A has a pH of 4.00. Solution B has a pH of 1.00. Which one is more acidic? How many times more acidic? b. CH3COOH and KCH3COO 0.027M c. H₂S and NaHS Acidic, Basic, or neutral 8. Whic of the owing combinations would act as buffered solutions (look at the ions individually)? JUSTIFY why. a. HCI and NaCl
Transcribed Image Text:Topic 14 HW 4. In each of the following chemical equations, identify the conjugate acid-base pairs. a. CH3NH2 + H₂O CH3NH3+ + OH- 5. Write a chemical equation showing how each of the following species can behave as indicated when dissolved in water(this is the other reactant). a. HSO3 as an acid A B 6. Complete the following table. Show all calculations in the open space, clearly labeled. Solution pH POH [H+] [OH-] PUO b. CH3COOH + NH3 CH3COO- + NH4+ C b. CO32- as a base D 9.63 1.22 3.9x10-6M 7. Solution A has a pH of 4.00. Solution B has a pH of 1.00. Which one is more acidic? How many times more acidic? b. CH3COOH and KCH3COO 0.027M c. H₂S and NaHS Acidic, Basic, or neutral 8. Whic of the owing combinations would act as buffered solutions (look at the ions individually)? JUSTIFY why. a. HCI and NaCl
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