Chapter 19 Notes
Honors Chemistry
Chapter 19: Acids, Bases, and Salts
Section 1 Notes – Acid Base Theories
(Read pages 587-593)
Acids
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Taste _________________________ or _________________________
Conduct electricity
Strong or weak electrolytes
_________________________
React with metals to form _________________________ gas
React with bases to form salt and water
Changes indicators (turns litmus paper _________________________)
Different Classifications of Acids
 _________________________
o Contains one ionizable hydrogen (Example: _________________________)
 _________________________
o Contains two ionizable hydrogens (Example: _________________________)
 _________________________
o Contains three ionizable hydrogens (Example: _________________________)
Bases
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Taste _________________________
Feels _________________________
Strong or weak electrolytes
Reacts with acids to form salt and water
Changes indicators (turns litmus paper _________________________)
Solutions sometimes known as _________________________
Three Definitions of Acids and Bases
 _________________________
 __________________________________________________
 _________________________
Arrhenius Acids and Bases
 Looks at acids and bases in terms of what they ____________________ in
__________________
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Chapter 19 Notes
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Honors Chemistry
Arrhenius Acid
o Produces ____________ or _____________ ions in _________________ solution
Arrhenius Base
o Produces _____________ ions in _________________________ solution
Bronsted-Lowry Acids and Bases
 Looks at acids and bases in terms of _______________________ ___________________
 Bronsted-Lowry Acid
o Donates a _________________________ (H+)
 Bronsted-Lowry Base
o Accepts a _________________________ (H+)
There’s something about water…
 Water is _________________________ or _________________________
 It can act as an _________________________ or _________________________
 Depends on what it is reacting with
Conjugate Acids and Bases
 Conjugate Acid
o Formed when a __________________ gains a _________________________ ion
 Conjugate Base
o Remains when an acid has _________________ a ______________________ ion
 Conjugate Acid-Base Pair
o Consists of 2 substances related by the _________________________ or
_________________________ of a single _________________________ ion
 Bases form conjugate _________________________
 Acids form conjugate _________________________
Lewis Acids and Bases
 Looks at acids and bases in terms of _________________________
 Lewis Acid
o _________________________ a pair of electrons to form a covalent bond
 Lewis Base
o _________________________ a pair of electrons to form a covalent bond
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Chapter 19 Notes
Honors Chemistry
Acid-Base Definitions (Summary)
Type
Arrhenius
Acid Definition
Base Definition
Bronsted-Lowry
Lewis
Section 2 Notes – Hydrogen Ions and Acidity
(Read pages 594-604)
Self-Ionization of Water
 Equation: H2O  H+ + OH Ion product constant of water = Kw = [H+][OH-] = _________________________
o This means that the ____________ and _____________ are equal to
_________________________ in a _________________________solution
o In an _________________________ solution, [H+] will be
_________________________ than [OH-]
o In a _________________________ solution, [OH-] will be greater than [H+]
 [ ] represents _________________________
Let’s Use It!
 Colas are slightly acidic. If the [H+] in a cola solution is 1.0 x 10-5 M, what is [OH-] in
the solution?
Practice Problems
1. If the hydroxide ion concentration of an aqueous solution is 1.0 x 10-3M, what is the
concentration of hydrogen ions in solution? Is the solution acidic, basic, or neutral?
2. Classify each of the following as acidic, basic, or neutral.
a. [H+] = 6.0 x 10-10 M
b. [OH-] = 3.0 x 10-2 M
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Chapter 19 Notes
Honors Chemistry
pH and pOH
 p represents the mathematical calculation of _________________________
_________________________ (or – log)
 So pH is _________________________ wheras pOH is _________________________
 pH + pOH = _________________________
o In a _________________________ solution, pH and pOH equal ________.
o In an _______________________ solution, pH is ___________________ than 7.
o In a ______________________ solution, pH is _____________________ than 7.
Two Examples
1. A solution has a pH of 12, what is the pOH of the solution?
2. If the [H+] of a solution is 3.4 x 10-10 M, what is the pH and pOH of the solution?
Practice Problems – Try it!
Find the pH and pOH of each of the following solutions. Classify each as acidic, basic, or
neutral.
1. Solution with an [H+] of 0.045 M
2. Solution with an [OH-] of 0.072 M
Finding [H+] and [OH-] from pH and pOH
 Remember that pH = -log [H+] so [H+] = _________________________
 This also applies to bases  [OH-] = _________________________
 Example: If a solution has a pH of 3.2, what is the [H+] in the solution?
Practice Problems
Find the [H+] and [OH-] for each of the following solutions:
1. A solution with a pH of 11.9
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Chapter 19 Notes
Honors Chemistry
2. A solution with a pOH of 12.4
Section 4 Notes – Neutralization Reactions
(Read pages 612-616)
Neutralization Reactions
 The reaction between an _________________________ and a
_________________________
 Products are _________________________ (ionic compound) and
_______________________
 Example: HCl + NaOH  NaCl + H2O
Titration
 A process used to determine the _________________________ of an
_________________________ or _________________________ solution in which a
standard solution of _________________________ concentration is added to a measured
amount of solution with an _________________________ concentration until an
_________________________ signals an _________________________
o Equivalence point – point in the titration where the number of moles of
_________________________ ions equals the number of moles of
_________________________ ions
Indicators
 Change ____________________ under different conditions of ____________________
 Help identify ______________________ and _________________________ solutions
 Many different indicators (Example: Phenolpthalein)
Titration Calculations – Finding the number of moles of acid or base required in a neutralization
1. How many moles of sulfuric acid are required to neutralize 0.50 mol of sodium
hydroxide?
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Chapter 19 Notes
Honors Chemistry
Practice Problems – You Try It!
1. How many moles of potassium hydroxide are needed to completely neutralize 1.56 mol
of phosphoric acid?
Titration Calculations – Determining an unknown concentration
1. A 25 mL of H2SO4 is completely neutralized by 18 mL of 1.0 M NaOH. What is the
concentration of the H2SO4 solution?
Practice Problems – Give It A Shot!
1. How many mL of 0.45 M HCl will neutralize 25.0 mL of 1.00 M KOH?
2. What is the molarity of H3PO4 if 15.0 mL is completely neutralized by 38.5 mL of 0.150
M NaOH?
And with that, you’ve officially completed all of the content
for intro. chem!! CONGRATS!
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