2. Suggest a maximum buffering capacity for each buffer. Look for their corresponding pkavalues first, you can find these in your textbooks or online sources (eg. Campbell'sBiochemistry, 9th ed).BufferingСараcityMaximumBufferingСараcityBuffer ComponentspK valueAmmonium/Ammonia bufferLactic acid/Lactate bufferPhosphoric acid/hydrogen PO4 bufferBenzoic acid/Benzoate bufferFollow-up question:Which of these buffers would you use if you need to carry out a PCR reaction usingTaq polymerase which has an optimum pH at 7.2? Suggest only one buffer.Answer:Why?

2. Suggest a maximum buffering capacity for each buffer. Look for their corresponding pka values first, you can find these in your textbooks or online sources (eg. Campbell's Biochemistry, 9th ed). Maximum Buffering Сараcity Buffer Components pK value Buffering Сараcity Ammonium/Ammonia buffer Lactic acid/Lactate buffer Phosphoric acid/hydrogen PO4 buffer Benzoic acid/Benzoate buffer Follow-up question: Which of these buffers would you use if you need to carry out a PCR reaction using Taq polymerase which has an optimum pH at 7.2? Suggest only one buffer. Answer: Why?

2. Suggest a maximum buffering capacity for each buffer. Look for their corresponding pka values first, you can find these in your textbooks or online sources (eg. Campbell's Biochemistry, 9th ed). Maximum Buffering Сараcity Buffer Components pK value Buffering Сараcity Ammonium/Ammonia buffer Lactic acid/Lactate buffer Phosphoric acid/hydrogen PO4 buffer Benzoic acid/Benzoate buffer Follow-up question: Which of these buffers would you use if you need to carry out a PCR reaction using Taq polymerase which has an optimum pH at 7.2? Suggest only one buffer. Answer: Why?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 107AP

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Similar questions

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.
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
A best buffer has about equal quantities of weak acid and conjugate base present as well as having a large concentration of each species present. Explain.
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.
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Calculate the pH after 0.010 mole of gaseous HCl is added to 250.0 mL of each of the following buffered solutions. a. 0.050 M NH3/0.15 M NH4Cl b. 0.50 M NH3/1.50 M NH4Cl Do the two original buffered solutions differ in their pH or their capacity? What advantage is there in having a buffer with a greater capacity?
8-58 What is the connection between buffer action and Le Chatelier's principle?
Which of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Cl
5. Which of the following could be added to a solution of monobasic dihydrogen phosphate (KH2PO4) to produce a buffer? Briefly explain your answer(s). Dibasic monohydrogen phosphate hydrochloric acid sodium chloride A) hydrochloric acid only B) sodium chloride only C) Dibasic monohydrogen phosphate (K2HPO4) only D) Dibasic monohydrogen phosphate (K2HPO4) and sodium chloride
ave to.) The K of acetic acid is 1.8 | 10. (Note: solid sodium acetate comes as a hydrate NaC2H3O2 3H2O), and thus has a molar mass of 135.08 g/mol.) Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic acid/acetate buffer at pH 4.10, given that you will use 5.00 mL of 1.0 M acetic acid.
Directions: Read and analyze the following questions and compute for is unknown in the given problem. 1. Calculate the pH of a buffer made up of 0.544M CH3NH2 and 0.678M CH:NH3°CI- Ka of CH:NH2 is 1.8 x 105. The buffer is made up of CH3NH2 (weak base) and CH3NH3 CI (salt or conjugate acid) 2. Calculate the pH of buffer made of 0.500M NH3 and 0.456M NH.CI, pKo NH3 = 4.74. 3. Calculate the pH of a buffer solution consisting of 0.96OM NH3 and 0.608M NH4". The Ko for NH3 = 1.8 x 105. The reaction is: NH3 + H2O = NH + OH" item 2 and 3
H8. Describe the difference between a buffered and an unbuffered solution. Explain the significance of a buffer solution in a real-life application. Provide a unique example in your discussion