posted by .

Ammonia,is a weak base with a Ka value of 1.8x10^-5 .What is the pH of a 0.22M ammonia solution?

What is the percent ionization of ammonia at this concentration?

I got the answer for PartA which is pH=11.3. but i cant slove PartB..HELP!!!


    Ammonia has a Kb of 1.8x10^-5 (NOT the Ka)
    Kb = [NH4+][OH-] / [NH3]
    Let [OH-] = [OH-] = x
    1.8x10^-5 = x^2/(0.22-x)
    We can get an adequate approximate solution by assuming
    1.8x10^-5 = x^2/(0.22)
    x = [OH-] = 0.00199
    pOH = -log(0.00199) = 2.7
    pH = 11.3 (your answer)
    The approximate % ionization is:
    [(0.00199) / (0.22)](100) = _______?


    thanx a tons =)

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chem II

    Ammonia is a weak base. If Ammonium nitrate is added to it, the pH of the ammonia solution will _____________ (increase, decrease, stay the same)
  2. Chemistry

    Ammonia has the formula NH3. Household ammonia is a dilute aqueous solution of NH3 . Aqueous ammonia is a base that can neutralize acids. If 18.4mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, …
  3. chem help

    Ammonia,is a weak base with a Ka value of 1.8x10^-5 .What is the pH of a 0.22M ammonia solution?
  4. chemistry

    I am doing a home lab experiment about acid-base neutralization. I just need a little help to see if I am doing it correctly. I completed the experiment and recorded the data. We were to add 25 ml of vinegar and the 1 ml of cabbage …
  5. chemistry

    4.The Kb of ammonia, NH3, is 1.8x10^-5. What is the pH of a 2.000 millimolar solution of ammonia , to 3 significant digits.
  6. Chemistry

    Ammonia, NH3 is freely soluble in water, and has the value Kb=1.8x10^-5. If the pH of an ammonia solution is 11.4272, then what original concentration of NH3 (molarity) was used to make up the solution?
  7. Chemistry

    A 51.46 mL sample of an ammonia solution is analyzed by titration with HCl. The reaction is given below. NH3(aq) + H+(aq) NH4+(aq) It took 38.57 mL of 0.0984 M HCl to titrate (react completely with) the ammonia. What is the concentration …
  8. Chemistry - Equilibrium

    You have an unknown concentration of ammonia. When you add 15.0mL of a 0.400 M HCl solution to 50.0mL of the ammonia solution, the pH of the solution becomes 8.75. What is the concentration of the original ammonia solution?
  9. Chemistry

    calculate the pH of a 0.2moldm-3 solution of ammonia at 298K given that Kb for ammonia is 1.8x10-5
  10. Chemistry - Science (Dr. Bob222)

    Ammonia is a weak base with a Kb of 1.8 x 10-5. A 100.0 mL sample of 0.13 M aqueous solution of ammonia (NH3) is mixed with 87 mL of 0.15 M solution of the strong acid HCl, calculate the pH of the final solution. A) 2.9 B) 11.1 C) …

More Similar Questions