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3. Which of the following is a good buffer system? a. A solution that is 0.10 M NaCl and 0.10 M HCl b. A solution that is 0.10 M HCN and 0.10 M LICN c. A solution that is 0.10 M NaOH and 0.10 M HNO3 d. A solution that is 0.10 M HNO3 and 0.10 M KNO3 e. A solution that is 0.10 M HCN and 0.10 M NaCl Explain the reason for your choice:

3. Which of the following is a good buffer system? a. A solution that is 0.10 M NaCl and 0.10 M HCl b. A solution that is 0.10 M HCN and 0.10 M LICN c. A solution that is 0.10 M NaOH and 0.10 M HNO3 d. A solution that is 0.10 M HNO3 and 0.10 M KNO3 e. A solution that is 0.10 M HCN and 0.10 M NaCl Explain the reason for your choice:

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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Name Show your work and circle the final answer. Use the reference sheets for all equilibrium constant values needed. choice. 1. Which of the following salts has the highest molar solubility in water? Explain the reason for your a) CuCO3 b) CaF2 c) Fe(OH)2 2. Suppose that you have a saturated solution of lead (II) bromide (PbBr2) at 25 °C. Through titration, it is determined that the saturated solution contains 0.435 g of lead(II) bromide in 100 mL of solution. What is the solubility product constant (Ksp) for PbBr2? 3. Which of the following is a good buffer system? a. A solution that is 0.10 M NaCl and 0.10 M HC1 b. A solution that is 0.10 M HCN and 0.10 M LICN c. A solution that is 0.10 M NaOH and 0.10 M HNO3 d. A solution that is 0.10 M HNO3 and 0.10 M KNO3 e. A solution that is 0.10 M HCN and 0.10 M NaCl Explain the reason for your choice: 4. A precipitate forms when a small amount of ammonia (NH3) is added to a solution of silver nitrate. This precipitate dissolves when more ammonia is added. a. What is the identity (formula) of the precipitate? b. Explain why the precipitate dissolves when more NH3 is added. 5. A sample of ammonia (NH3) is titrated with nitric acid (HNO3). Do you expect that the pH at the equivalence point will be neutral, basic, or acidic? Write an equation to explain why.
Transcribed Image Text:Name Show your work and circle the final answer. Use the reference sheets for all equilibrium constant values needed. choice. 1. Which of the following salts has the highest molar solubility in water? Explain the reason for your a) CuCO3 b) CaF2 c) Fe(OH)2 2. Suppose that you have a saturated solution of lead (II) bromide (PbBr2) at 25 °C. Through titration, it is determined that the saturated solution contains 0.435 g of lead(II) bromide in 100 mL of solution. What is the solubility product constant (Ksp) for PbBr2? 3. Which of the following is a good buffer system? a. A solution that is 0.10 M NaCl and 0.10 M HC1 b. A solution that is 0.10 M HCN and 0.10 M LICN c. A solution that is 0.10 M NaOH and 0.10 M HNO3 d. A solution that is 0.10 M HNO3 and 0.10 M KNO3 e. A solution that is 0.10 M HCN and 0.10 M NaCl Explain the reason for your choice: 4. A precipitate forms when a small amount of ammonia (NH3) is added to a solution of silver nitrate. This precipitate dissolves when more ammonia is added. a. What is the identity (formula) of the precipitate? b. Explain why the precipitate dissolves when more NH3 is added. 5. A sample of ammonia (NH3) is titrated with nitric acid (HNO3). Do you expect that the pH at the equivalence point will be neutral, basic, or acidic? Write an equation to explain why.
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