posted by .

for chemical equilibrium, what is the difference between percent ionization and percent dissociation

  • chemistry -

    None. Many people, and I include myself, misuse the two terms because we often use them interchangeably. Actually, they are not.
    Two examples.
    1. NaCl is a solid crystal that consists of Na^+ and Cl^- bound together in a crystal lattice. When this crystal is placed in water it dissolves and DISSOCIATES into the hydrated ions. Most of us say it ionized but actually it did not. Ions were already there; the ions already there dissociated from each other to from the hydrated ions in solution. Acetic acid, which has no ions in it (covalent bonds and pure acetic acid does not conduct electricity) reacts with water to form ions.
    CH3COOH + H2O ==> H3O^+ +_ CH3COO^- and we should say it ionized in solution because we took a material with NO ions and made ions from the molecule.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry, #5

    For propanioic acid, HC3H5O2, Ka=1.3 x 10^-5, determine the concentration of the species present, the pH and the percent dissociation of a 0.21 M solution. Do this for H+, OH-, C3H5O2-, HC3H5O2, and the pH and percent dissociation. …
  2. chemistry

    Calculate the Ka of nitrous acid if a 0.200 mol/L solution at equilibrium at SATP has a percent ionization of 5.8%
  3. chemistry

    What is the percent ionization of a 1.38 mol/L weak acid if its Ka = 2.7 x 10-6?
  4. math

    A bond has an average return of 6.8 percent and a standard deviation of 4.6 percent. What range of returns would you expect to see 68 percent of the time?
  5. chem

    Calculate the [h3o+] and [oh-], pH and the percent dissociation for both 0.25 mol/L HCl and 0.25 mol/L HCN. 0.25 mol/L HCL [H+] = 0.25 mol/L [OH-] = 1 x 10^-14 / 0.25 = 4 x 10^-14 pH = 0.60 % dissociation = ?
  6. ap chemistry

    For propanoic acid (HC3H5O2, Ka = 1.3 10-5), determine the concentration of all species present, the pH, and the percent dissociation of a 0.29 M solution. [H+] [C3H5O2-] [OH -] [HC3H5O2] pH percent dissociation
  7. chemistry

    For a week acid whose ionization constant is 1.75 x 10(-5), the pH of its solution is 3.0. Determine its degree of ionization and its percent ionization.
  8. Chemistry

    What will happen if a small amount of hydrochloric acid is added to a 0.1 M solution of HF?
  9. chemistry

    i need help solving this Benzoic acid is a weak, monoprotic acid (Ka = 6.3 × 10−5). Calculate the pH and the percent dissociation of each of the following solutions of benzoic acid. Then use Le Châtelier’s principle to explain …
  10. AP Chem

    Hey guys! Thanks for any help in advance! I'm back with this problem: Calculate the percent dissociation for a 1.00 × 10-6 M solution of HCN at 25 °C. Ka = 4.90 × 10-10. So my question really is do I have to use water when I calculate …

More Similar Questions