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Acids and Bases

Acids and Bases. Chapter 14. Some Properties of Acids. Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) Taste sour Corrode metals React with bases to form a salt and water pH is less than 7

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Acids and Bases

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  1. Acids and Bases Chapter 14

  2. Some Properties of Acids • Produce H+ (as H3O+) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) • Taste sour • Corrode metals • React with bases to form a salt and water • pH is less than 7 • Turns blue litmus paper to red “Blue to Red A-CID”

  3. Some Properties of Bases • Produce OH- ions in water • Taste bitter, chalky • Feel soapy, slippery • React with acids to form salts and water • pH greater than 7 • Turns red litmus paper to blue “Basic Blue”

  4. Acid/Base Definitions • Brønsted – Lowry Acids – proton donor Bases – proton acceptor A “proton” is really just a hydrogen atom that has lost it’s electron!

  5. Bronsted-Lowry Acids Acids are hydrogen ion (H+) donors Bases are hydrogen ion (H+) acceptors HCl + H2O H3O+ + Cl- donor acceptor + - + + LecturePLUS Timberlake

  6. Reactions of acids Copy the 7 reactions from pg 319

  7. Conjugate pairs An acid and a base which differ only by the presence or absence of a proton (H+ )are called a conjugate acid-base pair. One half of the pair is always on the left-hand side of the equation, the other on the right-hand side. conjugatebase conjugateacid base acid The stronger an acid, the weaker its conjugate base, and, conversely, the stronger a base, the weaker its conjugate acid.

  8. Conjugate Pairs

  9. Learning Check! Example 3.1 For each of the following acid/base reactions, link the conjugate acid/base pairs: a) HCl (aq) + H2O (l) ----> H3O+ (aq) + Cl- (aq) b) H2SO4 (aq) + H2O (l) ----> HSO4- (aq) + H3O+ (aq) c) NH3 (g) + H2O (l) ----> NH4+ (aq) + OH- (aq) d) H3O+ (aq) + OH- (aq) -----> 2 H2O (l)

  10. Ans. Solution acid/base base/acid a) HCl (aq) / Cl- (aq) H2O (l) / H3O+ (aq) b) H2SO4 (aq) / HSO4- (aq) H2O (l) / H3O+ (aq) c) H2O (l) / OH- (aq) NH3 (g) / NH4+ (aq) d) H3O+ (aq) / H2O (l) OH- (aq) / H2O (l)

  11. Strong and Weak Acids/Bases The strength of an acid (or base) is determined by the amount of IONIZATION. HNO3, HCl, HBr, HI, H2SO4 and HClO4 are the strong acids.

  12. Strong Acid Weak Acid 15.4

  13. STRENGTH OF ACIDS AND BASES The strength of an acid or base is determined by its percent dissociation/ionization in water. All strong acids and bases dissociate/ionize completely, 100%.

  14. Strong Acids • Hydrohalic acids: HCl, HBr, HI • Nitric acid: HNO3 • Sulfuric acid: H2SO4 • Perchloric acid: HClO4

  15. Weak Acids • *One of the best known is acetic acid CH3CO2H

  16. CaO Strong Bases Common strong bases include NaOH ,KOH andCa(OH)2. Strong bases are (—OH), oxides of 1A and 2A metals (except Mg and Be), H-, and .

  17. Weak Bases One of the best known weak bases is ammonia NH3 (aq) + H2O (l) ↔ NH4+ (aq) + OH- (aq)

  18. Polyprotic and amphiprotic • A polyprotic acid is one which is capable of donating more than one proton. • A polyprotic base is one which is capable of accepting more than one proton. • An amphiprotic (amphoteric) substance can act as either an acid or a base.

  19. Amphiprotic substances • Examples • Water acts as a base in its reaction with HCl and as an acid in its reaction with NH3. • NH3(aq) + H2O(l) ➝ NH4(aq) + OH–(aq) • HCl(g) + H2O(l) ➝ H3O+(aq) + Cl–(aq)

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