4. You need to make a buffer with pH as close to 10.00 as possible. Two sets of weak acidsand conjugate bases, with the Ka values, are listed below. Which of the two sets wouldbe the best choice? You want a pka close to the pH. Explain your reasoning.CH:COOH/CH;coo HCO; /CO,2-Ka = 1.80 x 10sKa = 2.14 x 10-10%3D%3D5. 5 drops of a strong base (0.1 M concentration) was added to a buffer (pH = 7.0), with noapparent change in pH. An additional 5 ml of this strong base was added, and the pH ofthe solution increased to 13.0. Explain why there was no apparent change in pH in the%3Dfirst case, but a marked change in pH in the second case.

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4. You need to make a buffer with pH as close to 10.00 as possible. Two sets of weak acids and conjugate bases, with the Ka values, are listed below. Which of the two sets would be the best choice? You want a pKa close to the pH. Explain your reasoning. CH3COOH/CH3COO HCO3 /CO;? Ka = 1.80 x 105 Ka = 2.14 x 10-10

4. You need to make a buffer with pH as close to 10.00 as possible. Two sets of weak acids and conjugate bases, with the Ka values, are listed below. Which of the two sets would be the best choice? You want a pKa close to the pH. Explain your reasoning. CH3COOH/CH3COO HCO3 /CO;? Ka = 1.80 x 105 Ka = 2.14 x 10-10

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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Acetic acid has a Ka of 1.8 x 10¬º. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: A. [acetic acid] ten times greater than [acetate], B. [acetate] ten times greater than [acetic acid], and C. [acetate] = [acetic acid]. Match each buffer to the expected pH. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help [acetate] ten times greater than [acetic acid] [acetate] = [acetic acid] [acetic acid] ten times greater than [acetate] pH = 3.74 pH = 4.74 pH = 5.74
a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF.The Ka for HF is 7.2×10-4. pH = b) Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3×10-7 Сoncentration = M c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka value of HA ? = d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 40.0 mL pH = 50.0 mL pH =
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please do only the highlighted qouestion
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