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Chapter 19 “Acids, Bases, and Salts”

Chapter 19 “Acids, Bases, and Salts”. electrolytes. Properties of Acids & Bases!. ACIDS. BASES. electrolytes. sour taste. bitter taste. turn litmus red. turn litmus blue. react with metals to form H 2 gas. don’t react w/metals. slippery feel. “clean” feel.

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Chapter 19 “Acids, Bases, and Salts”

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  1. Chapter 19“Acids, Bases, and Salts”

  2. electrolytes Properties of Acids & Bases! ACIDS BASES • electrolytes • sour taste • bitter taste • turn litmus red • turn litmus blue • react with metals to form H2 gas • don’t react w/metals • slippery feel • “clean” feel • vinegar, milk, soda, apples, citrus fruits • ammonia, lye, antacid, baking soda • pH < 7 • pH > 7 • Produce OH– ions in H2O • Produce H+ ions in H2O ChemASAP

  3. Properties • Electrolytes can conduct electricity • Can be strong or weak electrolytes in aqueous solution

  4. Acids have a pH less than 7

  5. Acids Affect Indicators Blue litmus paper turns red in contact with an acid.

  6. Acids React with Active MetalsAcids react with active metals to form salts and hydrogen gas:HCl(aq) + Mg(s)→ MgCl2(aq) + H2(g)How can you tell if the gas produced is hydrogen?

  7. Acids React with Carbonates 2HC2H3O2 + Na2CO3 2NaC2H3O2 + H2O + CO2

  8. Effects of Acid Rain on Marble(calcium carbonate) George Washington: BEFORE George Washington: AFTER

  9. Bases have a pH greater than 7

  10. Bases Affect Indicators Red litmus paper turns blue in contact with a base. Phenolphthalein turns purple in a base. Vid properties

  11. Different Acid & Base Definitions

  12. H H – + O O Cl Cl H H H H Definitions • Arrhenius - In aqueous solution (when dissolved in water)… • Acidsform hydronium ions (H3O+) (or H+) HCl+ H2O  H3O+ + Cl– acid Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  13. Arrhenius said: An acid can be defined as a substance that yields hydrogen ions (H+) when dissolved in water. HCl Pure, dry substance is hydrogen chloride When dissolved in water it’s hydrochloric acid… it breaks into H+ ions & Cl- ions

  14. A base can be defined as a substance that yields hydroxide ions (OH-) when dissolved in water. NaOH sodium hydroxide KOH potassium hydroxide Ba(OH)2 barium hydroxide 2.7

  15. H H – + N O O N H H H H H H H H Definitions Video 1 • Arrhenius - In aqueous solution… • Bases form hydroxide ions (OH-) NH3+ H2O  NH4+ + OH- base Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  16. conjugate base conjugate acid Definitions • Brønsted-Lowry • Acidsare proton (H+) donors. • Bases are proton (H+) acceptors. HCl + H2O  Cl– + H3O+ acid base Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  17. Acids and bases come in pairs • A “conjugate base” is the remainder of the original acid, after it donates it’s proton/hydrogen ion • A “conjugate acid” is the particle formed when the original base gains a proton/hydrogen ion • Indicators are weak acids or bases that have a different color from their original acid and base

  18. O N H O H O O H Definitions H2O + HNO3 H3O+ + NO3– B A CA CB Acid Base Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  19. Acids and bases come in pairs • Amphoteric – a substance that can act as both and acid and base- as water shows Video 2

  20. Definitions • Lewis –same guy who came up with the Lewis-dot structures • Acidsare electron pair acceptors. • Bases are electron pair donors. Lewis base Lewis acid Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  21. Acid Definitions The Arrhenius model of acids and bases was broadened by the Bronsted-Lowry model. The Bronsted-Lowry model was broadened by the Lewis model The Lewis acid-base model is the most general in scope. Lewis acids Bronsted-Lowry Arrhenius acids Ralph A. Burns, Fundamentals of Chemistry 1999, page 483

  22. Acid – Base Systems

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