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Acids and Bases

Acids and Bases. Types of Acids. Binary Acids (contains H & 1 other element) HCl- hydro chlor ic acid Oxyacids (contain H, O, & other elements) H 2 SO 4 H 2 SO 3. Common Acids. Sour milk (lactic acid) Vinegar (acetic acid) Carbonated beverages (phosphoric acid)

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Acids and Bases

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  1. AcidsandBases

  2. Types of Acids Binary Acids (contains H & 1 other element) • HCl-hydrochloric acid Oxyacids (contain H, O, & other elements) • H2SO4 • H2SO3

  3. Common Acids • Sour milk (lactic acid) • Vinegar (acetic acid) • Carbonated beverages (phosphoric acid) • Lemons, oranges (citric acid) • Apples (malic acid) • Grape Juice (tartaric acid)

  4. Most commonly used product in the world Petroleum Automobile batteries Dehydration agent Metallurgy Refining Sulfuric Acid

  5. Stains proteins yellow Suffocating odor Stains skin Causes burns Explosives Rubber Plastics Dyes Pharmaceuticals Nitric Acid

  6. Phosphoric Acid • Manufacturing fertilizers for plants and animal feed • Flavoring agent in beverages • Cleaning agent for dairy equipment

  7. Hydrochloric acid • Produced in the stomach • Cleaning agent • Maintain acidity in pools

  8. Common Properties of Acids • Sour taste • Produce hydronium H3O+ ions • Change the color of acid-base indicators • React with active metals to release hydrogen gas • React with bases to produce salts and water • Conduct electric current

  9. Bases

  10. Common Bases • Lye (sodium hydroxide) • Milk of magnesia (magnesium hydroxide) • Antacids (aluminum hydroxide)

  11. Common Properties of Bases • Taste bitter • Produce hydroxide OH- ions • Change the color of acid-base indicators • Feel slippery • React with acids to produce salts and water • Conduct electric current

  12. Specific Definitions of Acids/Bases

  13. Arrhenius Acids and Bases • Arrhenius acid-increases H+ ions (H3O+) H2SO4 + H2O H3O+ +HSO4- • Arrhenius base-increases OH- ions Ca(OH)2Ca+2 + 2OH-

  14. Weak/Strong • Weak acid-weak electrolyte (end in -COOH) • Strong acid-ionizes completely, strong electrolyte (HCl) • Alkaline-base completely dissociates in water to yield OH- ions NaOH  Na+ + OH- • Strong bases-completely dissociates, strong electrolyte (end in OH)

  15. Bronsted-Lowry • Bronsted-Lowry Acid-proton donor • Bronsted-Lowry Base-proton acceptor HCl + NH3NH4+ + Cl- • Monoprotic acid-donates one proton HCl • Diprotic acid-donates two protons H2SO4 • Triprotic acid-donates three protons H3PO4

  16. Conjugate Acids and Bases • Conjugate base-the species that remains after a Bronsted-Lowry acid has given up a proton HF + H2O  F- + H3O+ Acid Conj. Base • Conjugate acid-the species that is formed when a Bronsted-Lowry base gains a proton HF + H2O  F- + H3O+ Base Conj. Acid

  17. Strength of Acid/Conj. Base Strong acidweak conjugate base Weak acidstrong conjugate base

  18. Amphoteric compound-any species that can react as either and acid or a base • Neutralization-the reaction of hydronium ions and hydroxide ions to form water molecules and salt Self-ionization of water H3O+ + OH-2H2O or H20 + H2OH3O+ + OH- • Salt-an ionic compound composed of a cation from a base and an anion from an acid

  19. Titration Practice Problems

  20. Ex 1 A 30.mL volume of HCl is titrated with 23mL of 0.20M NaOH. What is the molarity of HCl in this solution?

  21. Answer 0.15M

  22. Ex 2 A 26mL volume of NaOH is titrated with 23mL of 0.20MHCl. What is the molarity of NaOH in this solution?

  23. Answer 0.18M

  24. Ex 3 A 40.mL volume of H2SO4 is titrated with 38mL of 0.24M NaOH. What is the molarity of H2SO4 in this solution?

  25. Answer 0.11M

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