A buffer solution is composed of 0.1 M CH3OOH and 0.2 M CH3COONaa.) What is the pH of this buffer?b.) If 10mL 0.1 M NaOH is added to 110 mL of this solution, what will be the pH?c.) If 15mL 0.12 M HCI is added to 120 mL of this solution, what will be the finalpH?d.) Prepare a graph illustrating the 3 pH levels computed. Insert the graph intothe space below. Briefly explain the meaning of the graph.

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Answered: A buffer solution is composed of 0.1 M…

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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a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a solution which is 0.40 M in NH4+ and 0.40 M in NH3? The Kb of NH3 is 1.8 x 10-5. The correct answer should be reported to two places past the decimal. b) Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.
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Suppose 90.00 mL of 0.200M HCl is added to an acetate buffer prepared by dissolving 0.100 mol of acetic acid and 0.110 mol of sodium acetate in 0.100 L of solution. What are the initial and final pH values? What would be the pH if the same amount of HCI solution were added to 190 mL of pure water? Initial pH = Final pH pH after HCl is added to water =
When a strong base like NaOH is added to an acetate buffer (CH3COOH + H₂O CH3COO¯ + H3O*) the pH will.. A) increase by more than 1 pH unit B) decrease by more than 1 pH unit C) increase slightly D) stay the same. The pH will not change at all.
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