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Properties of Acids and Bases

Properties of Acids and Bases. Topic 8.2. But first, a review!. Practice problems. Identify the acid, base, conjugate acid, conjugate base, and conjugate acid-base pairs:. HC 2 H 3 O 2 (aq) + H 2 O (l)  C 2 H 3 O 2 – (aq) + H 3 O + (aq). conjugate base. conjugate acid. acid. base.

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Properties of Acids and Bases

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  1. Properties of Acids and Bases Topic 8.2

  2. But first, a review!

  3. Practice problems Identify the acid, base, conjugate acid, conjugate base, and conjugate acid-base pairs: HC2H3O2(aq) + H2O(l)  C2H3O2–(aq) + H3O+(aq) conjugate base conjugate acid acid base conjugate acid-base pairs OH–(aq) + HCO3–(aq)  CO32–(aq) + H2O(l) base acid conjugate base conjugate acid conjugate acid-base pairs

  4. HF(aq) + SO32–(aq)  F–(aq) + HSO3–(aq) (a) conjugate base conjugate acid acid base conjugate acid-base pairs (b) CO32–(aq)+HC2H3O2(aq)C2H3O2–(aq)+HCO3–(aq) base acid conjugate base conjugate acid conjugate acid-base pairs (c) H3PO4(aq) + OCl–(aq)  H2PO4–(aq) + HOCl(aq) conjugate base conjugate acid acid base conjugate acid-base pairs

  5. 8a) HCO3–(aq) + S2–(aq)  HS–(aq) + CO32–(aq) conjugate acid conjugate base acid base conjugate acid-base pairs 8b) H2CO3(aq) + OH–(aq)  HCO3–(aq) + H2O(l) acid base conjugate base conjugate acid conjugate acid-base pairs 11a) H3O+(aq) + HSO3–(aq)  H2O(l) + H2SO3(aq) conjugate base conjugate acid acid base conjugate acid-base pairs 11b) OH–(aq) + HSO3–(aq)  H2O(l) + SO32–(aq) conjugate acid conjugate base base acid conjugate acid-base pairs For more lessons, visit www.chalkbored.com

  6. Properties of Acids • taste sour • cool to use in movies • corrode metals (produce H2 gas) • react with bases to form salt and water • pH is less than 7 • turns blue litmus paper to red • strong acids are strong electrolytes, weak acids are weak electrolytes

  7. Properties of Bases • produce OH- ions in solution (Arrhenius definition) • taste bitter • feel soapy, slippery • dissolve oil and grease • react with acids to form salt and H2O • pH is greater than 7 • turns red litmus paper to blue • strong bases are good electrolytes, weak bases weak electrolytes

  8. Bases in Solution • solublebasesare considered to be alkalis • when added to water release an OH-ion • base(aq) = alkali • K2O(s) + H2O(l)  2K+(aq) + 2OH-(aq) • NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq) • CO32-(aq) + H2O(l) ⇌ HCO3-(aq) + OH-(aq) • HCO3-(aq) ⇌ CO2(g) + OH-(aq)

  9. The 5 Reactions of Acids “swap the hydrogen for the metal”

  10. METAL OXIDE (base) METAL CARBONATE or HYDROGEN CARBONATE (base) BASES (without OH) METAL (if more reactive than hydrogen) METAL HYDROXIDE (base)

  11. 1. Acids reaction with metals • most dilute acids react with metals above hydrogen in the reactivity series to produce H2 gas and a solution of a salt • in general: • reactive metal + acid  salt + hydrogen • Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) • Mg(s) + 2HNO3(aq)  Mg(NO3)2(aq) + H2(g) • Mg(s) + H2SO4(aq)  MgSO4(aq) + H2(g) • Mg(s) + 2CH3COOH(aq)  (CH3COO)2Mg(aq) + H2(g)

  12. 2. Acid reaction with metal hydroxides • acids react to give salt and water when a metal hydroxide(OH) or aqueous ammonia is added • in general: • metal hydroxide + acid  salt + water • NaOH(aq) + HNO3(aq)  NaNO3(aq) + H2O(l)

  13. 3. Acid reaction with metal carbonates or hydrogen carbonates • acids react to give CO2(g) when a metal carbonate or metal hydrogen carbonate is added • in general • (metal)CO3 + acid  salt + water + carbon dioxide • (metal)HCO3+ acid  salt + water + carbon dioxide • CaCO3(s) + 2HCl(aq)  CaCl2(aq) + H2O(l) + CO2(g) • NaHCO3(s) + HCl  NaCl(aq) + H2O(l) + CO2(g)

  14. 4. Acid Reaction with metal oxides • acids react to give salt and water when a metal oxide is added: • in general: • metal oxide + acid  salt + water • CuO(s) + H2SO4(aq)  CuSO4(aq) + H2O(l) • CuO(s) + 2HNO3(aq)  Cu(NO3)2(aq) + H2O • CuO(s) + 2HCl(aq)  CuCl2(aq) + H2O(l) • CuO(s) + 2CH3COOH(aq)  Cu(CH3COO)2(aq) + H2O(l)

  15. 5. Acid reactions with bases without an OH • a base is a substance that reacts with an acid to form water and a salt only, this is known as neutralization • most have an OH, however some do not • in general: • base + acid  salt + water • NH3(aq) + HNO3(aq)  NH4NO3 • NH3(aq) + H+(aq)  NH4+(aq) • H3PO4(aq) + 3NaHCO3(s)  Na3PO4(aq) + 3H2O(l) + 3CO2(g) • CaCO3(s) + 2HCl(aq)  CaCl2(aq) + H2O(l) + CO2(g)

  16. METAL OXIDE (base) METAL CARBONATE or HYDROGEN CARBONATE (base) BASES (without OH) METAL (if more reactive than hydrogen) METAL HYDROXIDE (base)

  17. Acids and bases effects on indicators • indicators • substances that change color in an acid or base (concentration of hydrogen ions changes)

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