A buffer solution can be prepared by starting with a weak acid. HA, and converting some of the weak acid to its salt (for example. NaA) by titration with a strong base The fraction of the original acid that is converted to the salt is designated f. a. Derive an equation similar to equation (17.7) but expressed in terms off rather man concentrations b. What is the pl at the point in the titration of phenol C g H 5 OH , at which f=0.27 ( p K g of phenol − 10.00)?
A buffer solution can be prepared by starting with a weak acid. HA, and converting some of the weak acid to its salt (for example. NaA) by titration with a strong base The fraction of the original acid that is converted to the salt is designated f. a. Derive an equation similar to equation (17.7) but expressed in terms off rather man concentrations b. What is the pl at the point in the titration of phenol C g H 5 OH , at which f=0.27 ( p K g of phenol − 10.00)?
Solution Summary: The author explains that a buffer solution is prepared by converting weak acid HA to its salt, and the ratio of equilibrium is the same.
A buffer solution can be prepared by starting with a weak acid. HA, and converting some of the weak acid to its salt (for example. NaA) by titration with a strong base The fraction of the original acid that is converted to the salt is designated f. a. Derive an equation similar to equation (17.7) but expressed in terms off rather man concentrations
b. What is the pl at the point in the titration of phenol
C
g
H
5
OH
, at which f=0.27 (
p
K
g
of phenol − 10.00)?
Two buffers are prepared by adding an equal numberof moles of formic acid (HCOOH) and sodium formate(HCOONa) to enough water to make 1.00 L of solution.Buffer A is prepared using 1.00 mol each of formic acid andsodium formate. Buffer B is prepared by using 0.010 mol ofeach. (a) Calculate the pH of each buffer. (b) Which bufferwill have the greater buffer capacity? (c) Calculate thechange in pH for each buffer upon the addition of 1.0 mLof 1.00 M HCl. (d) Calculate the change in pH for each bufferupon the addition of 10 mL of 1.00 M HCl.
a). What are acids, bases and buffers?b) What are the different types of buffers? Describe the mechanism howbuffers resist pH change in a system.c) Elaborate all chemical reactions in the standardization of NaOH withKHP?d) Why do you need to use KHP in the standardization of NaOH?e) Why is phenolphthalein used as an indicator in this experiment?f) Compare and contrast: endpoint vs equivalence point.g) Discuss the role of acids, bases, buffers and pH in water qualitymonitoring and post-harvest fisheries.
Explain how does a solution butanoic acid and potassium butanoate can function as a buffer solution?
include a bief description of how this buffer function on the addition of (i) a small amount of acid , (ii) a small amount of alkali , (iii) a small amount of distilled water and include a balanced chemical equation, physical state included.
Chapter 17 Solutions
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