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

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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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
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.
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A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
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You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.