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Acids

Section 1 Properties of Acids and Bases. Chapter 14. Acids. 1. Aqueous solutions of acids have a ______ taste. 2. Acids change the ______ of acid-base indicators. 3. Some acids react with active metals and release _______________. Ba( s ) + H 2 SO 4 ( aq ) BaSO 4 ( s ) + H 2 ( g ).

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Acids

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  1. Section1 Properties of Acids and Bases Chapter 14 Acids • 1. Aqueous solutions of acids have a ______ taste. • 2. Acids change the ______ of acid-base indicators. • 3. Some acids react with active metals and release _______________. • Ba(s) + H2SO4(aq) BaSO4(s) + H2(g) • 4. Acids react with bases to produce ____ and _____. • 5. Acids conduct _________________.

  2. Visual Concepts Chapter 14 Properties of Acids

  3. Section1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature • A ____________ 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 _________. • 2. The root of the name of the second element follows this prefix. • 3. The name then ends with the suffix ____.

  4. Section1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature, continued

  5. Section 1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature, continued • An _________ 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 ______ are based on the names of the acids.

  6. Section1 Properties of Acids and Bases Chapter 14 Acids, continued Acid Nomenclature, continued

  7. 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. Diluted to become ___________.

  8. Section1 Properties of Acids and Bases Chapter 14 Bases • 1. Aqueous solutions of bases taste _________. • 2. Bases change the ______ of acid-base indicators. • 3. Dilute aqueous solutions of bases feel ________. • 4. Bases react with acids to produce ________. • and ________. • . • 5. Bases ________ electric current.

  9. Section1 Properties of Acids and Bases Chapter 14 Arrhenius Acids and Bases • An _________________ is a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution. • An _______________ is a substance that increases the concentration of hydroxide ions, OH−, in aqueous solution.

  10. Section1 Properties of Acids and Bases Chapter 14 Arrhenius Acids and Bases, continued Aqueous Solutions of Acids • Arrhenius acids are molecular compounds with __________ hydrogen atoms. • Their water solutions are known as _________ acids. • All aqueous acids are ___________.

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

  12. Section1 Properties of Acids and Bases Chapter 14 Arrhenius Acids and Bases, continued Strength of Acids • A ______________ is one that ionizes completely in aqueous solution. • a strong acid is a strong __________ • HClO4, HCl, HNO3 • A _____________ 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

  13. Section1 Properties of Acids and Bases Chapter 14 Arrhenius Acids and Bases, continued Aqueous Solutions of Bases • Most bases are ionic compounds containing metal __________ and the __________ anion, OH−. • dissociate in water • Ammonia, NH3, is molecular • Ammonia produces hydroxide ions when it reacts with _________ molecules.

  14. 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 _____________. • Strong bases are strong ___________.

  15. Section1 Properties of Acids and Bases Chapter 14 Relationship of [H3O+] to [OH–]

  16. Section2 Acid-Base Theories Chapter 14 Brønsted-Lowry Acids and Bases • A Brønsted-Lowry acid is a molecule or ion that is a ________________. • Hydrogen chloride acts as a Brønsted-Lowry acid when it reacts with ammonia. • Water can act as a Brønsted-Lowry acid.

  17. Section2 Acid-Base Theories Chapter 14 Brønsted-Lowry Acids and Bases, continued • A Brønsted-Lowry base is a molecule or ion that is a _____________________. • Ammonia _________ a proton from the hydrochloric acid. It acts as a Brønsted-Lowry base. • The OH− ion produced in solution by Arrhenius hydroxide bases (NaOH) is the Brønsted-Lowry base. • The OH− ion can accept a proton

  18. Section2 Acid-Base Theories Chapter 14 Brønsted-Lowry Acids and Bases, continued • In a Brønsted-Lowry acid-base reaction, protons are _________ from one reactant (the acid) to another (the base). acid base

  19. Section2 Acid-Base Theories Chapter 14 Monoprotic and Polyprotic Acids • A _____________ acid is an acidthatcan donate only one proton (hydrogen ion) per molecule. • HClO4, HCl, HNO3 • only one ionization step

  20. Section2 Acid-Base Theories Chapter 14 Monoprotic and Diprotic Acids

  21. Section2 Acid-Base Theories Chapter 14 Monoprotic and Polyprotic Acids, continued • A _________________ is an acid that can donate more than one proton per molecule. • H2SO4, H3PO4 • Multiple ionization steps • (1) • (2) • Sulfuric acid solutions contain H3O+, ions

  22. Section2 Acid-Base Theories Chapter 14 Monoprotic and Polyprotic Acids, continued • A diprotic acid is the type of polyprotic acid that can donate two protons per molecule • H2SO4 • A triprotic acid is the type of polyprotic acid that can donate three protons per molecule. • H3PO4

  23. Section2 Acid-Base Theories Chapter 14 Lewis Acids and Bases • A __________ is an atom, ion, or molecule that accepts an __________ to form a covalent bond. • The ____________ definition is the broadest of the three acid definitions. • A bare proton (hydrogen ion) is a Lewis acid

  24. Section2 Acid-Base Theories Chapter 14 Lewis Acids and Bases, continued • The formula for a Lewis acid need not include hydrogen. • The silver ion can be a Lewis acid • Any compound in which the central atom has three valence electrons and forms three covalent bonds can react as a Lewis acid.

  25. Section2 Acid-Base Theories Chapter 14 Lewis Acids and Bases, continued Acid Base Definitions

  26. Section3 Acid-Base Reactions Chapter 14 Conjugate Acids and Bases • The species that remains after a Brønsted-Lowry acid has given up a _________ is the conjugate base of that acid. acid conjugate base

  27. Section3 Acid-Base Reactions Chapter 14 Conjugate Acids and Bases, continued • Brønsted-Lowry acid-base reactions involve two acid-base pairs, known as conjugate acid-base pairs. acid1 base2 base1 acid2

  28. Section3 Acid-Base Reactions Chapter 14 Neutralization Reactions

  29. Section3 Acid-Base Reactions Chapter 14 Conjugate Acids and Bases, continued Strength of Conjugate Acids and Bases • The stronger an acid is, the weaker its conjugate base • The stronger a base is, the weaker its conjugate acid strong acid base acid weak base

  30. Section3 Acid-Base Reactions Chapter 14 Conjugate Acids and Bases, continued Strength of Conjugate Acids and Bases, continued • Proton transfer reactions favor the production of the _________ acid and the _________ base. • stronger acid stronger base weaker acid weaker base • The reaction to the _______ is more favorable • weaker acid weaker base stronger acid stronger base • The reaction to the ______ is more favorable

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

  32. Section3 Acid-Base Reactions Chapter 14 Amphoteric Compounds • Any species that can react as ___________________ is described as amphoteric. • example: water • water can act as a ______ • acid1 base2 acid2 base1 • water can act as an ______ • base1 acid2 acid1 base2

  33. Section3 Acid-Base Reactions Chapter 14 Amphoteric Compounds, continued –OH in a Molecule • The covalently bonded -OH group in an acid is referred to as a ______________. • Molecular compounds containing —OH groups can be_________ or _________. • The behavior of a compound is affected by the number of _________ atoms bonded to the atom connected to the —OH group.

  34. Section3 Acid-Base Reactions Chapter 14 Oxyacids of Chlorine

  35. Section3 Acid-Base Reactions Chapter 14 Neutralization Reactions Strong Acid-Strong Base Neutralization • In aqueous solutions, neutralization is the reaction of ___________ ions and ____________ ions to form water molecules. • A _______ is an ionic compound composed of a cation from a base and an anion from an acid.

  36. Section3 Acid-Base Reactions Chapter 14 Acid Rain • _________________________ gases from industrial processes can dissolve in atmospheric water to produce acidic solutions. • example: • Very acidic rain is known as ___________. • Acid rain can erode ________ and affect ___________.

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