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Chapter 17 Acid-Base Equilibria

Chapter 17 Acid-Base Equilibria. Brønsted-Lowry Acids. HNO 3 + H 2 O → H 3 O + + NO 3 -. Acid. Brønsted-Lowry Bases. Base. Acids and Bases. Arrhenius. HCl + H 2 O → H 3 O + + Cl -. NH 3 + H 2 O → NH 4 + + OH -. :. H. H. H. H. H. B. H. H. B. N. N. H. H. H. H.

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Chapter 17 Acid-Base Equilibria

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  1. Chapter 17Acid-Base Equilibria

  2. Brønsted-Lowry Acids HNO3 + H2O → H3O+ + NO3- Acid

  3. Brønsted-Lowry Bases Base

  4. Acids and Bases Arrhenius HCl + H2O → H3O+ + Cl- NH3+ H2O → NH4+ + OH-

  5. : H H H H H B H H B N N H H H H H Acids and Bases Lewis BH3 + NH3 →BH3NH3 Base Acid

  6. Examples of Lewis Acid and Bases Acid Base

  7. Conjugate Acid-Base Pairs

  8. Conjugate Acid-Base Pairs

  9. Multiprotic acids A B A B

  10. Multiprotic acids

  11. Ionization Constants for Acids

  12. Ionization Constants for Bases

  13. Molecular basis of acid/base strength

  14. Electron affinity

  15. Summary 3.2 × 10 5

  16. Concepts from Chapter 17 Definitions of acids and bases (Lewis, Brønsted and Arrhenius) Conjugate acid-base pairs Ionization constants (Ka, Kb, Kw) and ionization constant expressions pH, pOH, pKw, Factors contributing to acidity Solvent leveling The strong acids and strong bases (names and formulæ) Acid-base reactions (strong-strong, strong-weak, weak-strong, and weak-weak) Calculations Method of iterative approximation

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