1. MODERN CHEMISTRY CHAPTER 14 ACIDS AND BASES
Sections 1 -3
Properties of Acids & Bases
Acid-Base Theories Acid-Base Reactions
Chapter 14 Section 1 Properties of Acids-Bases p

2. Strong and Weak Electrolytes
Section 1 Compounds in Aqueous Solution
Chapter 14
Strong and Weak Electrolytes
Electrolytes are substances that yield ions and conduct an electric current in solution.
The strength with which substances conduct an electric current is related to their ability to form ions in solution.
Strong and weak electrolytes differ in the degree of ionization or dissociation.

3. Models for Strong and Weak Electrolytes and Nonelectrolytes
Section 1 Compounds in Aqueous Solution
Chapter 13
Models for Strong and Weak Electrolytes and Nonelectrolytes

4. Strong and Weak Electrolytes, continued
Section 1 Compounds in Aqueous Solution
Chapter 13
Strong and Weak Electrolytes, continued
Strong Electrolytes
A strong electrolyte is any compound whose dilute aqueous solutions conduct electricity well; this is due to the presence of all or almost all of the dissolved compound in the form of ions.
To whatever extent they dissolve in water, they yield only ions.
HCl, HBr, HI
All soluble ionic compounds

5. Ba(s) + H2SO4(aq) BaSO4(s) + H2(g)
Section 1 Properties of Acids and Bases
Chapter 14
Acids
1. Aqueous solutions of acids have a sour taste.
2. Acids change the color of acid-base indicators.
3. Some acids react with active metals and release hydrogen gas, H2.
Ba(s) + H2SO4(aq) BaSO4(s) + H2(g)
4. Acids react with bases to produce salts and water.
5. Acids conduct electric current.

6. Properties of Acids
Chapter 14 Section 1 Properties of Acids-Bases p

7. Chapter 14 Acids, continued Acid Nomenclature
Section 1 Properties of Acids and Bases
Chapter 14
Acids, continued
Acid Nomenclature
A binary acid is an acid that contains only two different elements: hydrogen and one of the more electronegative elements.
HF, HCl, HBr, and HI
Binary Acid Nomenclature
1. The name of a binary acid begins with the prefix hydro-.
2. The root of the name of the second element follows this prefix.
3. The name then ends with the suffix -ic.

8. Chapter 14 Acids, continued Acid Nomenclature, continued
Section 1 Properties of Acids and Bases
Chapter 14
Acids, continued
Acid Nomenclature, continued

9. Chapter 14 Acids, continued Acid Nomenclature, continued
Section 1 Properties of Acids and Bases
Chapter 14
Acids, continued
Acid Nomenclature, continued
An oxyacid is an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal.
HNO3, H2SO4
The names of oxyacids follow a pattern.
The names of their anions are based on the names of the acids.

10. Chapter 14 Acids, continued Acid Nomenclature, continued
Section 1 Properties of Acids and Bases
Chapter 14
Acids, continued
Acid Nomenclature, continued

11. Some Common Industrial Acids
Section 1 Properties of Acids and Bases
Chapter 14
Some Common Industrial Acids
Sulfuric Acid
Sulfuric acid is the most commonly produced industrial chemical in the world.
Nitric Acid
Phosphoric Acid
Hydrochloric Acid
Concentrated solutions of hydrochloric acid are commonly referred to as muriatic acid.
Acetic Acid
Pure acetic acid is a clear, colorless, and pungent-smelling liquid known as glacial acetic acid.

12. Chapter 14 Bases 1. Aqueous solutions of bases taste bitter.
Section 1 Properties of Acids and Bases
Chapter 14
Bases
1. Aqueous solutions of bases taste bitter.
2. Bases change the color of acid-base indicators.
3. Dilute aqueous solutions of bases feel slippery.
4. Bases react with acids to produce salts and water.
5. Bases conduct electric current.

13. Arrhenius Acids and Bases
Section 1 Properties of Acids and Bases
Chapter 14
Arrhenius Acids and Bases
An Arrhenius acid is a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution.
An Arrhenius base is a substance that increases the concentration of hydroxide ions, OH−, in aqueous solution.

14. Arrhenius Acids and Bases, continued
Section 1 Properties of Acids and Bases
Chapter 14
Arrhenius Acids and Bases, continued
Aqueous Solutions of Acids
Arrhenius acids are molecular compounds with ionizable hydrogen atoms.
Their water solutions are known as aqueous acids.
All aqueous acids are electrolytes.

15. Arrhenius Acids and Bases, continued
Section 1 Properties of Acids and Bases
Chapter 14
Arrhenius Acids and Bases, continued
Aqueous Solutions of Acids, continued
Common Aqueous Acids

16. Strong Acids MEMORIZE! HCl hydrochloric acid HI hydroiodic acid
An acid that ionizes completely in aqueous solution.
STRONG ACID LIST
HCl hydrochloric acid
HI hydroiodic acid
HBr hydrobromic acid
H2SO4 sulfuric acid
HNO3 nitric acid
HClO3 chloric acid
HClO4 perchloric acid
MEMORIZE!
Chapter 14 Section 1 Properties of Acids-Bases p

17. Weak Acids Carboxyl Group - COOH
An acid that releases few hydrogen ions in aqueous solution. - Dissociates slightly
A reversible reaction in equilibrium
Organic Acids
Carboxyl Group - COOH
Chapter 14 Section 1 Properties of Acids-Bases p

18. Properties of Bases
Chapter 14 Section 1 Properties of Acids-Bases p

19. Arrhenius Acids and Bases, continued
Section 1 Properties of Acids and Bases
Chapter 14
Arrhenius Acids and Bases, continued
Strength of Acids
A strong acid is one that ionizes completely in aqueous solution.
a strong acid is a strong electrolyte
HClO4, HCl, HNO3
A weak acid releases few hydrogen ions in aqueous solution.
hydronium ions, anions, and dissolved acid molecules in aqueous solution
HCN
Organic acids (—COOH), such as acetic acid

20. Arrhenius Acids and Bases, continued
Section 1 Properties of Acids and Bases
Chapter 14
Arrhenius Acids and Bases, continued
Aqueous Solutions of Bases
Most bases are ionic compounds containing metal cations and the hydroxide anion, OH−.
dissociate in water
Ammonia, NH3, is molecular
Ammonia produces hydroxide ions when it reacts with water molecules.

21. Arrhenius Acids and Bases, continued
Section 1 Properties of Acids and Bases
Chapter 14
Arrhenius Acids and Bases, continued
Strength of Bases
The strength of a base depends on the extent to which the base dissociates.
Strong bases are strong electrolytes

22. Strong and Weak Bases
Strong Bases – bases that dissociate completely – strong electrolytes
Formed from Group I & II metals
Weak Bases – bases that dissociate slightly – weak electrolytes
Example: Ammonia, NH3
NH3 + H2O  NH4+ + OH-
Chapter 14 Section 1 Properties of Acids-Bases p

23. Strong Acids & Bases
Chapter 14 Section 1 Properties of Acids-Bases p
p. 501

24. Relative Strengths of Acids and Bases
Section 3 Acid-Base Reactions
Chapter 14
Relative Strengths of Acids and Bases
Relative Strengths of Acids and Bases

25. Strong & Weak Acid & Base
Chapter 14 Section 1 Properties of Acids-Bases p
p. xx

26. Arrhenius Acids & Bases
Chapter 14 Section 1 Properties of Acids-Bases p

27. Neutralization Reactions
Section 3 Acid-Base Reactions
Chapter 14
Neutralization Reactions

28. Chapter 14 Amphoteric Compounds
Section 3 Acid-Base Reactions
Chapter 14
Amphoteric Compounds
Any species that can react as either an acid or a base is described as amphoteric.
example: water
water can act as a base
acid1 base2 acid base1
water can act as an acid
base acid acid base2

29. Amphoteric Compounds, continued
Section 3 Acid-Base Reactions
Chapter 14
Amphoteric Compounds, continued
–OH in a Molecule
The covalently bonded IOH group in an acid is referred to as a hydroxyl group.
Molecular compounds containing —OH groups can be acidic or amphoteric.
The behavior of a compound is affected by the number of oxygen atoms bonded to the atom connected to the —OH group.

30. Neutralization Reactions
Section 3 Acid-Base Reactions
Chapter 14
Neutralization Reactions
Strong Acid-Strong Base Neutralization
In aqueous solutions, neutralization is the reaction of hydronium ions and hydroxide ions to form water molecules.
A salt is an ionic compound composed of a cation from a base and an anion from an acid.

31. Section 3 Acid-Base Reactions
Chapter 14
Acid Rain
NO, NO2, CO2, SO2, and SO3 gases from industrial processes can dissolve in atmospheric water to produce acidic solutions.
example:
Very acidic rain is known as acid rain.
Acid rain can erode statues and affect ecosystems.

32. Visual Concepts
Chapter 14
Acid Precipitation