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Chapter 15

Chapter 15. Acids and Bases. Arrhenius Acid-Base Theory. Arrhenius, Svante August (1859-1927), Swedish chemist 1903 Nobel Prize in chemistry acid - proton donor base - hydroxide ion donor. Bronsted-Lowry Acid-Base Theory. acid - proton donor base - proton acceptor

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Chapter 15

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  1. Chapter 15 Acids and Bases Dr. S. M. Condren

  2. Arrhenius Acid-Base Theory Arrhenius, Svante August • (1859-1927), Swedish chemist • 1903 Nobel Prize in chemistry acid - proton donor base - hydroxide ion donor Dr. S. M. Condren

  3. Bronsted-Lowry Acid-Base Theory acid - proton donor base - proton acceptor strong vs. weak acids and bases • strong - completely ionized • weak - partially ionized Dr. S. M. Condren

  4. Acid-Base Reactions hydronium ion hydrated proton, H3O+ used interchangeably for H+ indicators natural or synthetic substance that changes color in response to the nature of its chemical environment. Dr. S. M. Condren

  5. Indicators • Indicators are used to provide information about the degree of acidity of a substance (pH) or the state of some chemical reaction within a solution being tested or analyzed. Dr. S. M. Condren

  6. Indicators • One of the oldest indicators is litmus, a vegetable dye that turns red in acid solutions and blue in basic ones. Other indicators include alizarin, methyl red, and phenolphthalein, each one being useful for a particular range of acidity or a certain type of chemical reaction. Dr. S. M. Condren

  7. Indicators Dr. S. M. Condren

  8. Neutralization Reactions acid + base ---> “salt” + water HCl + NaOH ---> NaCl + H2O Dr. S. M. Condren

  9. Sulfur Acid SO3 + H2O -----> H2SO4 Dr. S. M. Condren

  10. Phosphoric Acid P4O10(s) + 6H2O(l) ---> 4H3PO4(aq) Dr. S. M. Condren

  11. Strong vs. Weak Acids and Bases strong acid completely ionized weak acid partially ionized Dr. S. M. Condren

  12. Which of the following "molecular" pictures best represents a concentrated solution of the weak acid HA with Ka = 10-5? A, B Dr. S. M. Condren

  13. Autoionization of Water H2O + H2O <=> H3O+ + OH- [H3O+][OH-] K = ----------------- [H2O]2 Kw = K [H2O]2 = [H3O+][OH-] = 1.0 x 10-14 Dr. S. M. Condren

  14. Autoionization of Water Kw = K [H2O]2 = [H3O+][OH-] = 1.0 x 10-14 [H3O+][H3O+] = 1.0 x 10-14 [H3O+]2 = 1.0 x 10-14 [H3O+] = 1.0 x 10-7 -log([H3O+]) = -log(1.0 x 10-7) pH = -log([H3O+]) = 7.00 Dr. S. M. Condren

  15. pH Scale @ -2 -----> @ +16 pH = - log [H3O+] Dr. S. M. Condren

  16. A solution with pH=5 is 100 times more acidic than a solution with a pH =? 7, 3, 0.05 Dr. S. M. Condren

  17. pH Scale Dr. S. M. Condren

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