ThepK, value forHF is 3.14. Would a buffer prepared fromHF andNaF with a pH of 1.14 be considered to be an effective buffer?A buffer in which the mole ratio ofNaF toHF is 0.46 has a pH of 2.80. Would this buffer solution have a greater capacity foadded acid (H3O*) or added base (OH )?A buffer solution that is 0.425 M inCH, COOH and 0.425 M inCH3 COONA has a pH of 4.74.The addition of 0.01 mol of OH to 1.0 L of this buffer would cause the pH toThe capacity of this buffer for added H30 could be increased by the addition of 0.130mol

The pK, value for HF is 3.14. Would a buffer prepared from HF and NaF with a pH of 1.14 be considered to be an effective buffer? A buffer in which the mole ratio of NaF to HF is 0.46 has a pH of 2.80. Would this buffer solution have a greater capa added acid ( H30) or added base ( OH )?

The pK, value for HF is 3.14. Would a buffer prepared from HF and NaF with a pH of 1.14 be considered to be an effective buffer? A buffer in which the mole ratio of NaF to HF is 0.46 has a pH of 2.80. Would this buffer solution have a greater capa added acid ( H30) or added base ( OH )?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 65QAP: Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105)....

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Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with little pH change? Is it necessary that the concentrations of the weak acid and the weak base in a buffered solution be equal? Explain. What is the pH of a buffer when the weak acid and conjugate base concentrations are equal? A buffer generally contains a weak acid and its weak conjugate base, or a weak base and its weak conjugate acid, in water. You can solve for the pH by setting up the equilibrium problem using the K.a reaction of the weak acid or the Kb reaction of the conjugate base. Both reactions give the same answer for the pH of the solution. Explain. A third method that can be used to solve for the pH of a buffet solution is the HendersonHasselbalch equation. What is the HendersonHasselbalch equation? What assumptions are made when using this equation?
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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.
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A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
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