Understanding Acids and Bases: Key Concepts & Properties

1. MODERN CHEMISTRY CHAPTER 14ACIDSANDBASES Sections 1 -3 Properties of Acids & Bases Acid-Base TheoriesAcid-Base Reactions Chapter 14 Section 1 Properties of Acids-Bases p. 466-477

2. Section1 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 ionizationor dissociation.

3. Section1 Compounds in Aqueous Solution Chapter 13 Models for Strong and Weak Electrolytes and Nonelectrolytes

4. Section1 Compounds in Aqueous Solution Chapter 13 Strong and Weak Electrolytes, continued Strong Electrolytes • Astrong electrolyteis 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. Section1 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. 466-477

7. Section1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature • Abinary acidis 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. Section1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature, continued

9. Section1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature, continued • Anoxyacidis 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. Section1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature, continued

11. Section1 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. Section1 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. Section1 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. • AnArrhenius baseis a substance that increases the concentration of hydroxide ions, OH−, in aqueous solution.

14. Section1 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. Section1 Properties of Acids and Bases Chapter 14 Arrhenius Acids and Bases, continued Aqueous Solutions of Acids, continued • Common Aqueous Acids

16. Chapter 14 Section 1 Properties of Acids-Bases p. 466-477 Strong Acids • 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!

17. Chapter 14 Section 1 Properties of Acids-Bases p. 466-477 Weak Acids • An acid that releases few hydrogen ions in aqueous solution. - Dissociates slightly • A reversible reaction in equilibrium • Organic Acids • Carboxyl Group - COOH

18. Properties of Bases Chapter 14 Section 1 Properties of Acids-Bases p. 466-477

19. Section1 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 • Aweak acidreleases 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. Section1 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. Section1 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. Chapter 14 Section 1 Properties of Acids-Bases p. 466-477 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-

23. Strong Acids & Bases • p. 501 Chapter 14 Section 1 Properties of Acids-Bases p. 466-477

24. Section3 Acid-Base Reactions Chapter 14 Relative Strengths of Acids and Bases Relative Strengths of Acids and Bases

25. Strong & Weak Acid & Base • p. xx Chapter 14 Section 1 Properties of Acids-Bases p. 466-477

26. Arrhenius Acids & Bases Chapter 14 Section 1 Properties of Acids-Bases p. 466-477

27. Section3 Acid-Base Reactions Chapter 14 Neutralization Reactions

28. Section3 Acid-Base Reactions Chapter 14 Amphoteric Compounds • Any species that can react as either an acid or a base is described asamphoteric. • example:water • water can act as a base • acid1 base2 acid2 base1 • water can act as an acid • base1 acid2 acid1 base2

29. Section3 Acid-Base Reactions Chapter 14 Amphoteric Compounds, continued –OH in a Molecule • The covalently bonded IOH group in an acid is referred to as ahydroxyl 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. Section3 Acid-Base Reactions Chapter 14 Neutralization Reactions Strong Acid-Strong Base Neutralization • In aqueous solutions,neutralizationis the reaction of hydronium ions and hydroxide ions to form water molecules. • Asalt is an ionic compound composed of a cation from a base and an anion from an acid.

31. Section3 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 asacid rain. • Acid rain can erode statues and affect ecosystems.

32. Visual Concepts Chapter 14 Acid Precipitation