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Equilibrium in Acid-Base Systems

acids, bases, equilibrium, ionization, pH, electrolytes, reaction, concentration

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Equilibrium in Acid-Base Systems

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  1. Equilibrium in Acid-Base Systems 16.1b: Acid strength and equilibrium position

  2. Strengths of acids • Strong acids • ionize completely, strong electrolyte • reacts completely with water to form H3O+ • assume the [H3O+] is equal to the initial acid conc. • shown as >99% over the yield/equilibrium arrow • Strong Acids to know • HCl, HBr, HI, HClO4, H2SO4, HNO3 >99%

  3. Strengths of Acids • Weak Acids • compounds with acidic properties that ionizes partially in solution • weak electrolytes • can assume any acid not on the SA list is weak • Ex. acetic acid, lactic acid, citric acid • reacts partially with water to form relatively few H3O+ • must calculate [H3O+] since small amount of initial acid ionizes • shown as <50% over the yield/equilibrium arrow <50%

  4. Why are some H’s acidic? • acidic: • weak bonds • polar bonds • non-acidic • strong bonds • nonpolar bonds

  5. Bases • most make OH- ions • strong bases dissociate into OH- ions and metal ion • Ca(OH)2 Ca2+ + 2OH- • LiOH Li+ + OH- • weak bases take a H+ from water and make OH- • NH3 + H2O  NH4+ + OH- • C6H5NH2 + H2O  C6H5NH3+ + OH-

  6. Bases • Weak Bases • do not contain OH- • accepts H+ from H2O to make OH-

  7. Percent Ionization • also called %rxtn. with water • in acid-base sol’n theory, reaction with water means the same as ionization in water • the higher the conc. of the weak acid sol’n the lower its % ionization • if we know the pH or initial acid conc. of a weak acid solution we can calculate the % ionization

  8. Percent Ionization con’t • formula p = % ionization [HA] = initial conc. of weak acid

  9. Example • Orange juice has a citric acid concentration of 0.23M and at equilibrium 3.1% has reacted to form H3O+ . Calculate the [H3O+] • Solution • use formula to solve Plug in and solve for [H3O+ ]. or

  10. Homework • Textbook p721 #2-7, 9, 11, 13, 14

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