ess imporWhich of the following aqueous solutions are good buffer systems?(Select all that apply.)0.18 M acetic acid + 0.17 M sodium acetate0.27 M hydroiodic acid + 0.24 M potassium iodide0.32 M ammonium nitrate + 0.31 M ammoniaUse the References to0.12 M calcium hydroxide + 0.22 M calcium chloride0.37 M hypochlorous acid + 0.25 M potassium hypochloriteSubmit AnswerRetry Entire Group 7 more group attempts remainingues ir needed tо

A buffer solution is formed by the mixture of weak acid and its conjugate base or by the mixture of…

Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.18 M acetic acid + 0.17 M sodium acetate 0.27 M hydroiodic acid + 0.24 M potassium iodide 0.32 M ammonium nitrate + 0.31 M ammonia 0.12 M calcium hydroxide + 0.22 M calcium chloride 0.37 M hypochlorous acid + 0.25 M potassium hypochlorite

Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.18 M acetic acid + 0.17 M sodium acetate 0.27 M hydroiodic acid + 0.24 M potassium iodide 0.32 M ammonium nitrate + 0.31 M ammonia 0.12 M calcium hydroxide + 0.22 M calcium chloride 0.37 M hypochlorous acid + 0.25 M potassium hypochlorite

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 3ALQ

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Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
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.
7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?
Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 103 HONH2 Kb = 1.1 108 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. a. HCO2H b. HOBr c. KHCO2 d. HONH3NO3 e. (C2H5)2NH f. (C2H5)2NH2Cl g. HONH2 h. NaOBr
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?
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.