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Acids and Bases

Acids and Bases. Arrhenius Theory. Acids produce H + ions. Bases produce OH - ions. HCl g H + + Cl - NaOH g Na + + OH -. Bronsted -Lowry Theory. Acids donate protons Bases accept protons HCl (g) + H 2 O(l) g H 3 O + ( aq ) + Cl - ( aq ) acid base

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Acids and Bases

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  1. Acids and Bases

  2. Arrhenius Theory • Acids produce H+ ions. • Bases produce OH- ions. HCl g H+ + Cl- NaOH g Na+ + OH-

  3. Bronsted-Lowry Theory • Acids donate protons • Bases accept protons HCl(g) + H2O(l) g H3O+(aq) + Cl-(aq) acid base Acid + base g conjugate base +conjugate acid conjugate acid conjugate base

  4. Neutralization • NH3(g) + H2O(l) g NH4+(aq) + OH-(aq) • A conjugate base is formed when an acid gives up its proton. • A conjugate acid is formed when a base accepts a proton. base acid conjugate acid conjugate base

  5. Lewis Theory • Acids accept an electron pair (must have an empty orbital) • Bases donate an electron pair (must have at least one filled orbital) H H + H N H + H-O-H H N H + OH- H

  6. All acids and bases discussed so far are Lewis acids and bases. • Now we have some new possibilities. . . H F H F H N:+ B F  H N B F H F H F Lewis base Lewis acid

  7. amphoteric • A substance that can act as an acid or a base. • Water: HCl + H2O g H3O+ + Cl- acid base NH3 + H2O g NH4+ + OH- base acid

  8. Anhydrides- acids or bases that have had water removed • Acidic anhydrides- produce an acid when dissolved in water Acid rain: SO2(g) + H2O(l) g H2SO4(aq) • Basic anhydride- produces a base when dissolved in water Na2O(s) + H2O(l) g 2NaOH(aq)

  9. If a metal oxide, a base will form • If a nonmetal oxide, an acid will form Write the formula for the anhydride of HNO3 We must remove an H2O. 2HNO3 – H2O g N2O5 Complete the following equation: CaO + H2O  CO2 + H2O  Ca(OH)2 H2CO3

  10. Strong acids ionize completely HCl HBr HI H2SO4 HNO3 HClO3 HClO4 The stronger an acid, the weaker its conjugate base and visa versa.

  11. Polyprotic acids • have more than one hydrogen to ionize • Ex: H2SO4 – the second or third H+ ionizes weakly

  12. Strong bases KOH NaOH Mg(OH)2 (low solubility, but dissociates) Ca(OH)2 -the hydroxides of alkali metals and heavy alkali earth metals

  13. Naming acids anion acid name example -ide Hydro- ic HCl hydrochloric acid -ite -ous HNO2 nitrous acid -ate -ic HNO3 nitric acid

  14. H2SO4 HF H3PO4 H2SO3 H2CO3 HNO3 sulfuric acid hydrofluoric acid phosphoric acid sulfurous acid carbonic acid nitric acid Try these

  15. hydrolysis • The reaction of a salt with water to form an acidic or basic solution.

  16. Strong bases: hydroxides of groups 1 & 2 (except Be) • Strong acids: HCl, HBr, HI HClO3, HClO4, H2SO4, HNO3

  17. From NaOH, strong base From HCl, strong acid NaCl produces a neutral solution CuSO4 produces an acidic solution K2CO3 produces a basic solution H2SO4, strong acid A weak base KOH, Strong base Weak acid

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