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Acids and Bases Chapter 14

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Acids and Bases Chapter 14 Sections 4-7 Sample Exercise 14.7 Calculate the pH of 0.10 M HNO3 Calculate the pH of 1.0 x 10-10 M HCl Sample Exercise 14.8 The ... – PowerPoint PPT presentation

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Title: Acids and Bases Chapter 14


1
Acids and BasesChapter 14
  • Sections 4-7

2
Sample Exercise 14.7
  • Calculate the pH of 0.10 M HNO3
  • Calculate the pH of 1.0 x 10-10 M HCl

3
Sample Exercise 14.8
  • The hypochlorite ion (OCl-) is a strong oxidizing
    agent often found in household bleaches and
    disinfectants. It is also the active ingredient
    that forms when swimming pool water is treated
    with chlorine. In addition to its oxidizing
    abilities, the hypochlorite ion has a relatively
    high affinity for protons (it is a much stronger
    base than Cl- , for example) and forms the weakly
    acidic hypochlorous acid (HOCl, Ka 3.5 x 10-8).
    Calculate the pH of a 0.100M aqueous solution of
    hypochlorous acid.

4
Sample Exercise 14.9
  • Calculate the pH of a solution that contains 1.00
    M HCN (Ka 6.2 x 10-10) and 5.00 M HNO2 (Ka
    4.0 x 10-4). Also calculate the concentration of
    a cyanide ion (CN-) in this solution at
    equilibrium.

5
Sample Exercise 14.10
  • Calculate the percent dissociation of acetic acid
    (Ka 1.8 x 10-5) in each of the following
    solutions.
  • 1.00 M HC2H3O2
  • 0.100 M HC2H3O2

6
Sample Exercise 14.11
  • Lactic acid (HC3H5O3) is a waste product that
    accumulates in muscle tissue during exertion,
    leading to pain and a feeling of fatigue. In a
    0.100 M aqueous solution, lactic acid is 3.7
    dissociated, Calculate the vale of Ka for this
    acid.

7
Sample Exercise 14.12
  • Calculate the pH of 5.0 x 10-2 M NaOH solution.

8
Sample Exercise 14.13
  • Calculate the pH for a 15.0 M solution of NH3 (Kb
    1.8 x 10-5)

9
Sample Exercise 14.14
  • Calculate the pH of a 1.0 M solution of
    methylamine (Kb 4.38 x 10-4)

10
Polyprotic Acids
  • Dissociate in a step wise manner
  • Each successive Ka value for dissociation
    equilibria are Ka1 and Ka2
  • Ka1 gt Ka2 gt Ka3
  • INSERT TABLE 14.4 page 651
  • Only the first dissociation step makes an
    important contribution to H
  • EXCEPTSulfuric Acid is strong in the first
    dissociation and weak in the second dissociation.
    SO the second dissociation does make a
    contribution to H.

11
Sample Exercise 14.15
  • Calculate the pH of a 5.0 M H3PO4 solution and
    the equilibrium concentration of the species
    H3PO4, H2PO41-, HPO42-, PO43-

12
Sample Exercise 14.16
  • Calculate the pH of a 1.0 M H2SO4 solution.

13
Sample Exercise 14.17
  • Calculate the pH of a 1.00 x 10-2 M H2SO4
    solution.
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