The pH of 300 mL solution made of 0.63 M acetic acid and 0.96 M potassium acetate is (K₂ = 1.8 x 10-5) after the addition of 0.04 moles HCI Your Answer: Answer The pH of 300 mL solution made of 0.57 M acetic acid and 0.95 M potassium acetate is (K₂ = 1.8 x 10-5) after the addition of 0.095 moles NaOH Your Answer: Answer

The pH of 300 mL solution made of 0.63 M acetic acid and 0.96 M potassium acetate is (K₂ = 1.8 x 10-5) after the addition of 0.04 moles HCI Your Answer: Answer The pH of 300 mL solution made of 0.57 M acetic acid and 0.95 M potassium acetate is (K₂ = 1.8 x 10-5) after the addition of 0.095 moles NaOH Your Answer: Answer

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 30QRT

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Similar questions

8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to hit a titration end point? Explain.
8-68 If you have 100 mL of a 0.1 M buffer made of NaH2PO4 and Na2HPO4 that is at pH 6.8 and you add 10 mL of 1 M HCI, will you still have a usable buffer? Why or why not?
8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?
8-94 Suppose you wish to make a buffer whose pH is 8.21. You have available 1 L of 0.100 M NaH2PO4 and solid Na2HPO4. How many grams of the solid Na2HPO4 must be added to the stock solution to accomplish this task? (Assume that the volume remains 1 L.)
Metacresol purple is an indicator that changes from yellow to purple at pH 8.2. (a) What is Ka for this indicator? (b) What is its pH range? (c) What is the color of a solution with pH 9.0 and a few drops of metacresol purple?
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.
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
1. What is the pH after 25.0 ml of 0.100 M NaOH has been added to 50.0 ml of 0.100 M HCl? 1.00 1.48 7.00 13.00