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Intro to Acids & Bases

Intro to Acids & Bases. Ions in Solution. ____________ – contain more H + than OH - ____________ – contain more OH - than H + ____________ – contain equal amounts of H + and OH -. Autoionization of Water. H 2 O + H 2 O  H 3 O + + OH - Water is the usual solvent for acids and bases

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Intro to Acids & Bases

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  1. Intro to Acids & Bases

  2. Ions in Solution • ____________ – contain more H+ than OH- • ____________ – contain more OH- than H+ • ____________ – contain equal amounts of H+ and OH-

  3. Autoionization of Water • H2O + H2O  H3O+ + OH- • Water is the usual solvent for acids and bases • It produces equal numbers of H3O+ and OH-

  4. Arrhenius Model of Acids & Bases • ____________ - a substance that contains H and ionized to produce H+ when dissolved in water. • ____________ - a substance that contains OH and ionizes to produce OH- when dissolved in water

  5. Arrhenius Model of Acids & Bases • HCl • NaOH

  6. Arrhenius Model of Acids & Bases • Although the Arrhenius model is useful in describing many acids and bases, it does not describe them all • For example NH3 contains no OH- ions, but it is a base

  7. Bronsted-Lowry Model • ____________ - proton donor • ____________ - proton acceptor

  8. Bronsted-Lowry Model • ____________ – the species produced when a base accepts the H+ ion from the acid • ____________ – the species produced when the acid gives up its H+

  9. Conjugate Acids & Conjugate Bases • Identify the acid, base, conjugate acid, and conjugate base of the following reaction… • HX + H20  H3O+ + X-

  10. Conjugate Acids & Conjugate Bases • Identify the acid, base, conjugate acid, and conjugate base of the following reaction… • NH3 + H20  NH4+ + OH-

  11. Conjugate Acids & Conjugate Bases • ____________ – substance that can act as either an acid or a base

  12. Conjugate Acids & Conjugate Bases • Identify the acid, base, conjugate acid, and conjugate base of the following reactions… • NH4+ + OH- NH3 + H20 • HBr + H2O  H3O+ + Br -

  13. What are the conjugate bases of the following acids? HCl  H2SO4  What are the conjugate acids of the following bases? BrO2- NH3  Conjugate Acids & Conjugate Bases

  14. Monoprotic & Polyprotic Acids • ____________ – an acid that can only donate 1 H+ ion • For example – HCl, HBr, HNO3, HClO4 • ____________ – acids that can donate more than one H+ ion • For example – H2SO4, H3PO4

  15. Complete Ionization • Write the steps for the complete ionization of H2Se

  16. Complete Ionization • Write the steps for the complete ionization of H3AsO

  17. The pH Scale • [H+] is often expressed in very small numbers. • ____________ is a mathematical scale in which the concentration of hydronium ions in a solution is expressed as a number from 0 to 14.

  18. Interpreting the pH Scale • pH of 7 is neutral. A pH less than 7 is acidic, and a pH greater than 7 is basic.

  19. pH and pOH • The pH of a solution equals the negative logarithm of the hydrogen ion concentration

  20. pH and pOH • Calculate the pH of a solution whose [H+] is 1.0 x 10 -2 M

  21. More Examples • Calculate the pH of a solution whose [H+] is 3.0 x 10 -6 M • Calculate the pH of a solution whose [H+] is 8.2 x 10 -6 M

  22. More Formulas pH + pOH = 14 pH = - log [H+] pOH = - log [OH-] [H+] = antilog - pH [OH-] = antilog - pOH [H+][OH-] = 1 x 10 -14

  23. Examples • Calculate the pH, pOH, & [H+] of the following • [OH-] = 1.0 x 10 -6 M • Calculate the pH, pOH, & [OH-] of the following • [H+] = 3.6 x 10 -9 M

  24. Examples • Calculate the [OH-] if the [H+] is 1.0 x 10-5M

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