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Reactions in Aqueous Solutions I

Reactions in Aqueous Solutions I. Properties of Aqueous Solutions of Acids & Bases. Acidic properties taste sour change the colors of indicators turn litmus red react with metals to generate H 2(g) react with carbonates and bicarbonates to form salts, carbon dioxide and water

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Reactions in Aqueous Solutions I

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  1. Reactions in Aqueous Solutions I

  2. Properties of Aqueous Solutions of Acids & Bases Acidic properties • taste sour • change the colors of indicators • turn litmus red • react with metals to generate H2(g) • react with carbonates and bicarbonates to form salts, carbon dioxide and water • aqueous solutions conduct electricity • react with bases to produce salt and water

  3. Properties of Aqueous Solutions of Acids & Bases Basic properties • taste bitter • feel slippery • change colors of indicators • turn litmus blue • react with acids to form salts and water • aqueous solutions conduct electricity SOAP

  4. Arrhenius Acid • Acid - A substance that produces hydrogen ions, H+, in aqueous solutions. HCl H+ + Cl- HCN H+ + CN-

  5. Arrhenius Base • Base - A substance that produces hydroxide, OH-, in aqueous solutions. KOH K+ + OH- NH3 + H2O NH4+ + OH-

  6. Arrhenius Theory • neutralization - combination of H+ (or H3O+) with OH- • strong acids - ionize 100% in water HCl, HBr, HI, H2SO4, HNO3, HClO4 • strong bases - ionize 100% in water LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

  7. Arrhenius Theory • total ionic equation for strong acid with strong base

  8. Arrhenius Theory • net ionic equation for strong acid with strong base

  9. Acid-Base Theories • The most general theory for common aqueous acids and bases is the BRØNSTED - LOWRY theory • ACIDS DONATE H+ IONS • BASES ACCEPTH+ IONS

  10. Acid-Base Theories • ACIDS DONATE H+ IONS • BASES ACCEPTH+ IONS

  11. Brønsted-Lowry Acid-Base Theory • differences between Arrhenius & Brønsted-Lowry theories • reaction does not have to occur in an aqueous solution • bases do not have to be hydroxides • for example- ammonia is not a hydroxide NH3 + H2O NH4+ + OH-

  12. Hydronium Ion • The hydrated hydrogen ion or hydronium ion gives aqueous solutions of acids their characteristic acidic properties. H2O + H+H3O+ hydronium ion

  13. Hydrated Hydrogen Ion • H+(aq) is really H(H2O)n+ • n is a small integer = 7? • H3O+is usually used where n = 1 H3O+  H+

  14. Acid-Base Characteristics • Solution Type Relationship • Acid [H+ ] > [OH-] • Neutral [H+ ] = [OH-] • Base [H+ ] < [OH-]

  15. Brønsted–Lowry Acids • An acid is a proton donor. HNO3 + H2O H3O+ + NO3-

  16. Brønsted–Lowry Bases • A base is a proton acceptor. NH3 + H2O NH4+ + OH-

  17. Brønsted–Lowry Acids and Bases • The Brønsted definition means NH3 is a BASE in water — and water is itself an ACID.

  18. acid1 base2 Brønsted–Lowry Acids and Bases • An acid–base reaction is the transfer of a proton from an acid to a base. HCl + H2O H3O+ + Cl-

  19. Brønsted–Lowry Acids and Bases • When an acid gives up a proton, a conjugate base is formed that is capable of accepting a proton.

  20. acid1 base2 acid2 base1 Brønsted–Lowry Acids and Bases HF + H2O H3O+ + F-

  21. Conjugate Acid-Bases • Conjugate acid-base pairs are a reactant and a product that differ by a proton, H+.

  22. Conjugate Acid-Bases • Conjugate acid-base pairs are a reactant and a product that differ by a proton, H+.

  23. Conjugate Acid-Bases • Every acid has a conjugate base, formed by the removal of a proton from the acid. • Every base has a conjugate acid associated with it, formed by the addition of a proton to the base. • Thus H3O+ is the conjugate acid of H2O.

  24. Acid Base Conjugate acid Conjugate base Conjugate Acid-Bases HNO2 + H2O  H3O+ + NO2-

  25. Base Acid Conjugate base Conjugate acid Conjugate Acid-Bases NH3 + H2O  NH4+ + OH-

  26. Conjugate Acid–Base Strengths • The more readily a substance gives up a proton, the less readily its conjugate base accepts a proton. • The more readily a base accepts a proton, the less readily its conjugate acid gives up a proton.

  27. Conjugate Acid–Base Strengths • The stronger an acid, the weaker its conjugate base. • The weaker an acid, the stronger its conjugate base.

  28. Conjugate Acid–Base Strengths

  29. acid1 base2 acid2 base1 Ampholytes • A substance capable of being an acid or a base is amphoteric. H2O + H2O  H3O+ + OH-

  30. Bronsted-Lowry Acid-Base Theory • water can be either an acid or base in Bronsted-Lowry theory • amphoteric - species that can be either an acid or base • amphiprotic- proton transfer reactions that species behave as either an acid or base

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