The pH of a solution made from a 0.75 M acetic acid solution and a 0.54 M sodium acetate solution is (K, = 1.8 x 10-5) Your Answer: Answer Question 7 1) Listen The pH of 300 mL solution made of 1.10 M acetic acid and 0.80 M potassium acetate is (Ka = 1.8 x 105) after the addition of 0.03 moles HCI Your Answer: Answer Question 8 1) Listen The pH of 300 mL solution made of 0.97 M acetic acid and 1.19 M potassium acetate is (Ką = 1.8 x 10-5) after the addition of 0.010 moles NaOH Your Answer: Answer

The pH of a solution made from a 0.75 M acetic acid solution and a 0.54 M sodium acetate solution is (K, = 1.8 x 10-5) Your Answer: Answer Question 7 1) Listen The pH of 300 mL solution made of 1.10 M acetic acid and 0.80 M potassium acetate is (Ka = 1.8 x 105) after the addition of 0.03 moles HCI Your Answer: Answer Question 8 1) Listen The pH of 300 mL solution made of 0.97 M acetic acid and 1.19 M potassium acetate is (Ką = 1.8 x 10-5) after the addition of 0.010 moles NaOH Your Answer: Answer

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 95AP

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Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 103 HONH2 Kb = 1.1 108 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. a. HCO2H b. HOBr c. KHCO2 d. HONH3NO3 e. (C2H5)2NH f. (C2H5)2NH2Cl g. HONH2 h. NaOBr
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
You add 0.979 g of Pb(OH)2 to 1.00 L of pure water at 25 C. The pH is 9.15. Estimate the value of Ksp for Pb(OH)2.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.