The document outlines the properties of acids, bases, and salts, highlighting their observable characteristics, including taste, conductivity, and reactions with each other and metals. It introduces the pH scale to measure acidity and discusses models for understanding acids and bases, such as the Arrhenius, Bronsted-Lowry, and Lewis models. It also covers naming conventions for different types of acids and bases, neutralization reactions, and the titration process for determining concentrations.

1. Acids, Bases, and Salts
Rev Book Topic 10
Text Chapt 19

2. Properties of Acids and
Bases
 Certain observations can be made to
identify acids and bases
 These observable properties don’t
explain why acids and bases behave
the way they do.

3. Characteristic Properties of
Acids
 Dilute solutions of acids taste sour
 Lemons - citric acid
 Vinegar - acetic acid
 Pop - carbonic or phosphoric acid

4. Characteristic Properties of
Acids
 Aqueous solutions of acids conduct
current
 Recall… substances that conduct an
electric current are called electrolytes.
 If a solution of acid is a good conductor,
we call that acid a strong acid.
 If a solution of acid is a poor conductor,
we call it a weak acid.

5. Characteristic Properties of
Acids
 Acids react with bases to form water
and a salt.
 This is called a neutralization reaction
(a type of double replacement reaction).
 The salt formed is an ionic substance
composed of polyatomic or metallic
cation and an anion other than the
hydroxide ion.

6. Characteristic Properties of
Acids
 Acids react with certain metals to
produce hydrogen gas.
 Table J

7. Characteristic Properties of
Acids
 Acids cause acid-base indicators to
change color.
 Table M

8. Characteristic Properties of
Bases
 Bases have a bitter taste
 Bases have a slippery or “soapy” feeling
 Bases conduct an electric current
 Bases react with acids to produce
water and a salt
 Bases cause acid base indicators to
change color.

9. Reference Tables
 Table K - Common Acids
 Table L - Common Bases
 Table M - Indicators
 Table J - Activity Series

10. pH Scale
 A scale called the pH Scale expresses [H+
]
as a number from 0 to 14.
 A pH of 0 (zero) is strongly acidic.
 A pH of 7 is neutral
 A pHof 14 is strongly basic

11. pH Scale
 The pH scale is logarithmic. Each
change of a single pH unit represents
a tenfold change in the concentration
of hydrogen ion.
pH = - log [H+
]
[H+
] = 10-pH

12. pH Scale
 A solution with a pH of 4 has a [H+
]
that is ten times greater than that of
a solution with pH of 5.

13. Chemistry Lab
Acid Base pH mystery

14. Models of Acids and Bases
 We need to attempt to develop
explanations for the observable properties
of acids and bases.
 Three models have been developed…
 Arrhenius model
 Bronsted-Lowry Model
 Lewis Model

15. Worksheet
Models of Acids and Bases

16.  Acids that produce a single hydrogen
ion are called monoprotic acids
 HCl
 Acids that produce two hydrogen
ions are called diprotic acids.
 H2SO4
 Acids that produce three hydrogen
ions are called triprotic acids.
 H3PO4

17. Naming Acids and Bases
 Binary acids are composed of
hydrogen and one other element.
 Names of binary acids begin with hydro-
followed by the name of the other
element modified to end with -ic.
 HCl = “hydrochloric acid”

18. Naming Acids and Bases
 Ternary acids are molecular
substances that produce hydrogen
ions when dissolved in water and
consist of an oxygen containing
polyatomic anion
 -ate becomes -ic
 -ite becomes -ous

19. Naming Acids and Bases
 Bases are easy…
 Name of the positive ion, then add
hydroxide.

20. Let’s Practice
 Review Book Page 178 #14 and #15
 Same Page #3 - 9

21. Neutralization Reactions
 Let’s write the neutralization reaction
between Nitric Acid and sodium hydroxide.
 All neutralization reactions have same net
equation.
 In all neutralization reactions, there is a 1:1
ratio between moles of H+
and moles OH-

22. Titration
 Process used to determine the
unknown concentration of an acid or
base by adding measured volumes of
an acid or base of known
concentration
 The solution of known concentration is
called the standard solution.

23. Titration
 Let’s revisit molarity
Molarity = moles/volume
Or
Moles = molarity X volume

24. Titration
 In a neutralization reaction, the moles of
H+
must equal the moles of OH-
.
 Therefore,
Molarityacid x Volumeacid = Molaritybase X Volumebase
(Reference Tables Table T)

25. Titration
 Only catch is… we need a way to
know when we’ve reached neutral.
How can we know this???
 Indicators
 pH probes

26. Titration
 Let’s dot the I’s and cross the T’s….
 Units - the volume can be expressed as mL
(but you must be consistent on both sides)
 Molarity - is strictly speaking the
concentration of H+
or OH-
, not necessarily
the concentration of the acid or base.