5. (17.28 Brown) A buffer contains 0.15 mol of propionic acid (C2H5COOH) and 0.10 mol of sodiumpropionate (C2H5COONa) in 1.20 L. Ka=1.3x10-5a. What is the pH of this buffer?b. What is the pH of the buffer after the addition of 0.010 mol NaOH?C. What is the pH of the buffer after the addition of 0.010 mol of HI?

In the context of a buffer solution containing propionic acid (C2H5COOH) and its conjugate base,…

Answered: 5. (17.28 Brown) A buffer contains 0.15…

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 buffer which contains 0.50 mol pyruvic acid and 0.45 mol sodium pyruvate dissolved in 1.0 L of water has a pH of 2.34. Assuming no significant changes to volume, calculate the pH when 0.10 mol of NaOH is added to the buffer. (The pk of pyruvic acid is 2.39) A. 2.34 B. 13.00 C. 2.15 D. 2.52 E. How do I do this? [base] pH=pKa + log. [acid]
A biochemistry student wants to make an acidic buffer with pH of 4.20. They will start with 250 mL of a 0.5 M acetic acid (HC2H3O2) solution. Acetic acid has a pka of 4.75. There are two ways to make this buffer. 1.1 The student is given 250 mL of a 0.5 M acetic acid (HC2H;O2) solution. What mass (in g) of sodium acetate (NaC,H;O2: 82.03 g/mol) should they add to make this a solution with pH of 4.20? Round your answer to 3 significant digits. Assume that dissolving the solid will not change the volume of the solution. g of Nac,H;O2 1.2 The lab is currently out of sodium acetate. A friend suggests using sodium hydroxide. How does adding sodium hydroxide to an acetic acid solution make a buffer solution? Explain using a chemical equation. No calculation needed.
Consider a buffer made by adding 132.8 g of NaC-H5O, to 300.0 mL of 1.97 M HC-H.O, (Ka = 6.3 x 10-5) a. What is the pH of this buffer? b. What is the pH of the buffer after 0.750 mol of H+ has been added? c. What is the pH of the buffer after 0.250 mol of OH- has been added?
A buffer made up of equal volumes (403.6 mL) of each of 0.828 M A H and 0.898 M A minus. What is p H of the buffer after addition of 11.42 mL of 0.238 M N a O H? K a of A H is 6.910E-5. Answer: (4.203)
9:26 A buffer solution contains 0.274 M C,HgNH3Br and 0.386 M C,H5NH2 (aniline). Determine the pH change when 0.093 mol HBr is added to 1.00 L of the buffer. pH after addition – pH before addition = pH change =
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
Which of the following chemicals would be the best buffer for a pH 9.00 solution: NH3 (Kb = 1.75x10-5), C6H5NH2 (Kb = 3.99x10-10), H2NNH2 (Kb = 3.00x10-6), C5H5N (Kb = 1.69x10-9)? Group of answer choices C5H5N H2NNH2 C6H5NH2 NH3
#5 Find the pH of a buffer that consists of 0.25 M HBrO and 0.43 M KBrO (pKa of HBrO = 8.64). pH =
5. Which of the following acid-base systems is NOT suitable to prepare a buffer with a pH 7.4? MTS88,0 MACELI A. Tris (tris(hydroxymethyl)aminomethane): pKa = 8.0 3. Phosphate: pKal = 2.16 pKa2 = 7.21 pka3 = 12.32 C. Leucine: pKal= 2.328, pKa2=9.744 D. HEPES (4-(2-hydroxyethyl)-1-piperazineethanesulfonic acid): pKal = 3.0, pKa2 = 7.5

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