2nd Edition

ISBN: 9781305079243

Author: Steven S. Zumdahl, Susan A. Zumdahl

Publisher: Cengage Learning

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Chapter 14, Problem 13Q

An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity.

(a) Chapter 14, Problem 13Q, An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker , example 1

(b) Chapter 14, Problem 13Q, An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker , example 2

(c) Chapter 14, Problem 13Q, An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker , example 3

(d) Chapter 14, Problem 13Q, An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker , example 4

(e) Chapter 14, Problem 13Q, An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker , example 5

a. Is the acid a weak or strong acid? How can you tell?

b. Arrange the beakers in order of what the contents would look like as the titration progresses.

c. For which beaker would pH = pK_a? Explain your answer.

d. Which beaker represents the equivalence point of the titration? Explain your answer.

e. For which beaker would the K_a value for the acid not be necessary to determine the pH? Explain your answer.

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Chapter 14, Problem 12Q

Chapter 14, Problem 14Q

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a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…

Chapter 14 Solutions

Chemistry: An Atoms First Approach

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