Bundle: Chemistry: An Atoms First Approach, 2nd, Loose-Leaf + OWLv2, 4 terms (24 months) Printed Access Card

2nd Edition

ISBN: 9781305717633

Author: Steven S. Zumdahl, Susan A. Zumdahl

Publisher: Cengage Learning

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Textbook Question

Chapter 14, Problem 4RQ

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 acid–conjugate base or weak base–conjugate 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

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Chapter 14, Problem 3RQ

Chapter 14, Problem 5RQ

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A series of carbonic acid or carbonate buffers regulate pH in blood within the human body. The kidneys and the lungs work together to help maintain a blood pH of 7.4 by affecting the components of the buffers in the blood. What conjugate acid/base pair is the main component in the buffer? Write out the chemical reaction that the conjugate pair undergoes in water. What is the ratio of the acid to the base? What is the ideal pH range for this buffer? Is the pH of blood within the ideal range of the buffer? If it is not, what is the physiological reason that the body would have for still using a carbonate buffer as opposed to another conjugate pair?

A student must make a buffer solution with a pH of 7.00.7.00. Determine which weak acid is the best option to make a buffer at the specified pH. acetic acid, ?a=1.75×10−5,�a=1.75×10−5, 5.00 M propionic acid, ?a=1.34×10−5,�a=1.34×10−5, 3.00 M ammonium citrate, ?a=4.06×10−7,�a=4.06×10−7, 2.00 M sodium dihydrogen phosphate monohydrate, ?a=6.23×10−8,�a=6.23×10−8, 2.00 M Determine which conjugate base is the best option to make a buffer at the specified pH. sodium acetate trihydrate, CH3COONa⋅3H2OCH3COONa⋅3H2O disodium hydrogen phosphate heptahydrate, Na2HPO4⋅7H2ONa2HPO4⋅7H2O sodium propionate, CH3CH2COONaCH3CH2COONa sodium citrate dihydrate, C6H5O7Na3⋅2H2OC6H5O7Na3⋅2H2O The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 7.00? mass = g Based on this information, what…

A buffer is made using 100.0 mL of 0.100 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M NACH3 CH2 COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LIOH is added tot he buffer? What would be the effect on the [H+]?

Chapter 14 Solutions

Bundle: Chemistry: An Atoms First Approach, 2nd, Loose-Leaf + OWLv2, 4 terms (24 months) Printed Access Card

Ch. 14 - What is meant by the presence of a common ion? How...Ch. 14 - Define a buffer solution. What makes up a buffer...Ch. 14 - Prob. 3RQ Ch. 14 - A good buffer generally contains relatively equal...Ch. 14 - Prob. 5RQ Ch. 14 - Prob. 6RQ Ch. 14 - Sketch the titration curve for a weak acid...Ch. 14 - Sketch the titration curve for a weak base...Ch. 14 - What is an acidbase indicator? Define the...Ch. 14 - Prob. 10RQ

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Solution Summary: The author explains the behavior of a buffer that has equal concentration of weak acid-conjugate base and good buffering capacity.

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