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I. Introduction to Acids & Bases

Ch. 18 – Acids & Bases. I. Introduction to Acids & Bases. Review – Acid Nomenclature. Review – Acid Nomenclature. Review – Naming Acids. HCl H 2 S H 2 SO 4 H 2 SO 3 HNO 3 HNO 2 HBr. Hydrochloric acid Hydrosulfuric acid Sulfuric acid Sulfurous acid Nitric acid Nitrous acid

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I. Introduction to Acids & Bases

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  1. Ch. 18 – Acids & Bases I. Introduction toAcids & Bases

  2. Review – Acid Nomenclature

  3. Review – Acid Nomenclature

  4. Review – Naming Acids • HCl • H2S • H2SO4 • H2SO3 • HNO3 • HNO2 • HBr • Hydrochloric acid • Hydrosulfuric acid • Sulfuric acid • Sulfurous acid • Nitric acid • Nitrous acid • Hydrobromic acid

  5. electrolytes electrolytes A. Properties ACIDS BASES • bitter taste • sour taste • turn litmus red • turn litmus blue • react with metals to form H2 gas • slippery feel • vinegar, milk, soda, apples, citrus fruits • ammonia, lye, antacid, baking soda

  6. HF H3PO4 H2SO4 B. Definitions • Monoprotic – an acid with one H+ • Polyprotic – an acid with more than one H+ • Diprotic – an acid with 2 H+ • Triprotic – an acid with 3 H+ monoprotic triprotic diprotic polyprotic

  7. H H – + O O Cl Cl H H H H B. Definitions • Arrhenius • Acids contain hydrogen • Acidsform hydronium ions (H3O+) in aqueous solution HCl+ H2O  H3O+ + Cl– acid

  8. B. Definitions • Arrhenius • Bases contain a hydroxide group • Bases form hydroxide ions (OH-) in aqueous solution H2O NaOH Na+ + OH- base

  9. conjugate base conjugate acid B. Definitions • Brønsted-Lowry • Acidsare proton (H+) donors • Bases are proton (H+) acceptors HCl + H2O  Cl– + H3O+ acid base

  10. conjugate base conjugate acid B. Definitions • Brønsted-Lowry • Conjugate Acidsare the result after a base accepts a hydrogen ion • Conjugate Bases are the result after an acid donates a hydrogen ion HBr + NaOH  NaBr + H2O acid base

  11. B. Definitions H2O + HNO3 H3O+ + NO3– B A CA CB H2O + NH3 NH4+ + OH- B CA CB A • Amphoteric – can be an acid or a base

  12. F - H2PO4- H2O HF H3PO4 H3O+ B. Definitions • Give the conjugate base for each of the following: • Polyprotic – an acid with more than one H+

  13. Br - HSO4- CO32- HBr H2SO4 HCO3- B. Definitions • Give the conjugate acid for each of the following:

  14. B. Definitions • Lewis • Acidsare electron pair acceptors • Bases are electron pair donors Lewis base Lewis acid

  15. - + C. Strength • Strong Acid/Base • 100% ionized in water • strong electrolyte NaOH KOH KOH RbOH CsOH Ca(OH)2 Ba(OH)2 HCl HNO3 H2SO4 HBr HI HClO4

  16. - + C. Strength • Weak Acid/Base • does not ionize completely • weak electrolyte HF CH3COOH H3PO4 H2CO3 HCN NH3

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