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buffer

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.2: Controlling Ph: Buffer Solutions

Problem 4RC: 4. To prepare a buffer containing CH3CO2H and NaCH3CO2 and having a pH of 5, the ratio of the...

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Question

What is the pH of a buffer solution containing 0.40 M HA (pKa = 4.0) and 0.3 M NaA, and what would the pH be after adding 25 mL of 0.2 M NaOH to 85 mL of buffer solution?

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Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
6. If 25.1 mL of 0.109M acid with a pKa of 5.27 is titrated with 0.108 M NaOH solution, what is the pH of the titration mixture after12.0 mL of base solution is added?
What is the pH a buffer solution containing 0.35 M acetic acid and 0.39 M sodium acetate where the pKa of acetic acid is 4.75?
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What is the pH of a buffer that is .1 Molar in H2CO3 and 1M in NaHCO3?
Acetate buffers are used in biochemical studies of enzymes and other chemicalcomponents of cells to prevent pH changes that might change the biochemicalactivity of these compounds. Calculate the pH of an acetate buffer that is amixture with 0.10 M acetic acid and 0.10 M sodium acetate. Ka is 1.8 x 10-5.
What is the pH of a buffer that results when 5.46 mole of H3PO4 is mixed with 2.97 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are Ka1 = 7.5 × 10–3, Ka2 = 6.2 × 10–8, and Ka3 = 3.6 × 10–13)
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