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Chapter 19

Chapter 19. Acids and Bases. TEKS. (G) define acids and bases and distinguish between Arrhenius and Bronsted-Lowry definitions and predict products in acid base reactions that form water;

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Chapter 19

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  1. Chapter 19 Acids and Bases

  2. TEKS • (G) define acids and bases and distinguish between Arrhenius and Bronsted-Lowry definitions and predict products in acid base reactions that form water; • (H) understand and differentiate among acid-base reactions, precipitation reactions, and oxidation-reduction reactions; • (I) define pH and use the hydrogen or hydroxide ion concentrations to calculate the pH of a solution; and

  3. Properties of Acids and Bases Acids Bases Tastes bitter Slippery conducts electricity Turns red litmus blue Reacts with an acid to produce salt and water Has a pH above 7 • Tastes sour • reacts with metals to produce hydrogen gas • Reacts with carbonates to produce carbon dioxide • conducts electricity so are good electrolytes • Turns blue litmus red • Has a pH between 0-6 • Reacts with a base to produce salt and water

  4. Ions in Solution

  5. Arrhenius vsBronstead-Lowry

  6. Amphoteric Substances • Amphoteric- a substance that can act as both acids and bases • Ex: Water • When HF dissolves in water, water acts as base • When NH3 dissolves in water, water acts as acid

  7. Strong Acids vs Weak Acids • http://www.mhhe.com/physsci/chemistry/chang7/esp/folder_structure/ac/m2/s1/index.htm

  8. 19.2 Strengths of Acids

  9. Strong Base vs Weak Base • http://www.mhhe.com/physsci/chemistry/chang7/esp/folder_structure/ac/m2/s2/index.htm

  10. 19.2 Strengths of Bases

  11. 19.3 What is pH? • Pure water contains equal numbers of H+ and OH- ions • Kw = [H+] [OH-] • Use 1.0x10-14Mfor Kw

  12. Ion Product Constant of Water • Ion Product Constant of Water- Kw- the value of the equilibrium constant for water • At 298 K, Kw is 1.0 x 10-14 • Kw = [H+] [OH-]

  13. pH • pH- the negative logarithm of the hydrogen ion concentration • pH = -log [H+]

  14. Math Calculations • pH + pOH = 14 • pH= -log(H+) • pH when given pOH = 14- (-log OH)

  15. pH Scale • pH below 7 is an acid • pH above 7 is a base • pH = 7 is neutral

  16. pH of Common Substances Timberlake, Chemistry 7th Edition, page 335

  17. pH Scale • http://www.purchon.com/chemistry/flash/ph.swf

  18. 19.4 Neutralization • Neutralization Reaction- acid & base react to produce a salt & water • a Double-Replacement Reaction • Salt- an ionic compound formed from the cation of a base & anion of an acid

  19. Acid-Base Indicator- a compound that changes color as it is placed in either an acid or base

  20. Titration • The process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration.

  21. End Point • The point at which an indicator used in a titration changes color

  22. Buffers • A solution that resists changes in pH when limited amounts of acids and bases are added.

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