IONIC

• Process by which a compound in its molten (dissolved in medium) is broken down in its individual ionic components

  Ionization
• Certain covalent compounds such as HC2H3O2, NH4OH, etc undergo partial ionization when in water solutions.
• Established between ionized and non-ionized molecules.

  Equilibrium
• When dissolved in water or any other ionizing medium produced electrically charged particles called ions.

  Electrolytes
• Compounds whose water solutions conduct electricity due to the presence of ions.

  Electrolytes
• • Dissolve as molecules only
  • No ions are produced in water
  • Do not conduct an electric current


  Nonelectrolytes
• 2 kinds of electrolytes

  • strong electrolytes
  • weak electrolytes
• • substance whose water solution is completely ionized(100%)
  • they have more ions in water than weak electrolytes
  • good conductor of electricity


  Strong electrolytes
• • substances whose water solution are partially (or incompletely ionized in water solution)
  • they have few ions in water
  • poor conductor of electricity


  Weak electrolytes
• equilibrium constant describing the ionization of a weak acid or base

  Ionization Constant (Ki)
• A measure of the extent of ionization

  Degree of Ionization (∝)
• Acid - defined as a proton donor (Bronsted Lowry Theory)


  Ionization of Weak Acids ( Ka)
• Kinds of weak acids:

  • Monoprotic weak acid
  • Polyprotic weak acids
• Those that yield only one H+ upon ionization

  Monoprotic weak acid
• Those that yield more than one H + upon ionization

  Polyprotic weak acids
• Phenomenon wherein the dissociation of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion common with the weak electrolyte


  COMMON – ION EFFECT
• The effect upon the addition of a substance ( strong electrolyte- salt solution) which furnishes an ion that is common on what is produced on the ionization of a weak electrolyte

  COMMON – ION EFFECT
• • solution that resists a change in pH upon adding small amounts of acid or base
  • mixture of weak electrolyte and its salt which by common-ion effect maintains a nearly constant hydronium ion concentration when a strong acid or strong base is added
  • The principle involved in buffer solutions is the common ion effect

  BUFFERED SOLUTION
• Amount of acid or base the buffer can neutralize before pH begins to change

  Buffer capacity
• Two types of Buffer:

  • Acid buffer
  • Base buffer