Sample student prepares three buffer solutions. Each solution is 1.0 M inone of the acids in the table and 1.0 M in its corresponding sodium salt.Which of the solutions has the greatest buffer capacity with respect toadded NaOH and why?H.H.CIH CH-C-CH-CC=C0-HH.0-H0-HBenzoic AcidChloroacetic AcidFormic AcidKapKa6.2 x 10-54.2114 x 10-32.861.8 x 103.75The formic acid buffer because it donates both of its hydrogen atomsThe chloroacetic acld buffer becauseitis the strongest acidAll are the sameThe benzolc acd butfer because lis testongestecid

When NaOH is added to the the buffer solutions , it will react with acidic part of buffer. So the…

Sample student prepares three buffer solutions. Each solution is 1.0 M in one of the acids in the table and 1.0 M in its corresponding sodium salt. Which of the solutions has the greatest buffer capacity with respect to added NAOH and why? H. H. CI H-C H-C- H-C C=C 0-H H. 0-H 0-H H. H. Benzoic Acid Chloroacetic Acid Formic Acid Ka pKa 6.2 x 10-5 14 x 10-3 2.86 1.8 x 104 3.75 4.21 The formic acid buffer because it donates both of its hydrogen atoms The chloroacetic acid buffer because itis the strongest acid All are the same The benzoic acd butfer becatse ltis testrongestacid

Sample student prepares three buffer solutions. Each solution is 1.0 M in one of the acids in the table and 1.0 M in its corresponding sodium salt. Which of the solutions has the greatest buffer capacity with respect to added NAOH and why? H. H. CI H-C H-C- H-C C=C 0-H H. 0-H 0-H H. H. Benzoic Acid Chloroacetic Acid Formic Acid Ka pKa 6.2 x 10-5 14 x 10-3 2.86 1.8 x 104 3.75 4.21 The formic acid buffer because it donates both of its hydrogen atoms The chloroacetic acid buffer because itis the strongest acid All are the same The benzoic acd butfer becatse ltis testrongestacid

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.7QAP

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Similar questions

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 acidconjugate base or weak baseconjugate 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
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Calculate the pH after 0.15 mole of solid NaOH is added to 1.00 L of each of the following solutions: a. 0.050 M propanoic acid (HC3H5O2, Ka = 1.3 105) and 0.080 M sodium propanoate b. 0.50 M propanoic acid and 0.80 M sodium propanoate c. Is the solution in part a still a buffer solution after the NaOH has been added? Explain.
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
Consider die titration of 50.0 mL of 0.10 M H3A (Ka1 = 5.0 104, Ka2 = 1.0 108, Ka3 = 1.0 1012) titrated by 0.10 M KOH. a. Calculate the pH of the resulting solution at 125 mL of KOH added. b. At what volume of KOH added does pH = 3.30? c. At 75.0 mL of KOH added, is the solution acidic or basic?
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
A 50.0-mL sample of a 0.100 M solution of NaCN is titrated by 0.200 M HCl. Kb for CN is 2.0 105. Calculate the pH of the solution: a prior to the start of the titration; b after the addition of 15.0 mL of 0.200 M HCl; c at the equivalence point; d after the addition of 30.0 mL of 0.200 M HCl.
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105) with 0.100 M HCl.