posted by .

Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations

A) 0.377 M
B) 0.107 M
C) 4.16*10^-2 M

Ka= 1.9*10^-5

  • CHM -

    ..........HN3 ==> H^+ + N3^-

    Ka = (H^)(N3^-)/(HN3)
    Subtitute and solve for x = (H^+). Then % ion = [(H^+)/(HN3)]*100 = ?

    Watch the lower cncns; they may require solving a qudratic.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Calculate the percent ionization of benzoic acid at the following concentrations: 0.00014 M i got 68% but it says its wrong
  2. Chemistry

    The Ka of hydrazoic acid (HN3) is 1.9 × 10-5 at 25°C. What is the pH of a 0.35-M aqueous solution of HN3?
  3. Chemistry

    4.54 g of hydrazoic acid ( HN3 ) is added to water to make a final solution of 504 ml. What is the pH of the solution ?
  4. chemistry

    If the system below is at equilibrium in a closed vessel and a small amount of nitrous acid [HNO2(§¤)] is added, what would be expected to happen?
  5. Chemistry

    Calculate the percent ionizationof a 0.15 M benzoic acid solution in pure water Nd also in a solution containing 0.10M sodium benzoate. Why does the percent ionization differ significantly in the two solutions?
  6. chemistry

    A 0.185 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.
  7. Chemistry

    The following questions refer to the following acids and bases. A) Hydrazoic acid HN3 Ka = 1.9 x 10^-5 B) Hydrofluoric acid HF Ka = 6.8 x 10 ^-4 C) Nitrous Acid HNO2 Ka = 4.5 x 10^-4 D) Phenol C6H5OH Ka = 1.3 x 10^-10 E) Aniline C6H5NH2 …
  8. 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 …
  9. chemistry

    a) Calculate the percent ionization of 0.125M lactic acid (Ka=1.4x10^-4) b) Calculate the percent ionization of 0.125M lactic acid in a solution containing 0.00075 M sodium lactate.
  10. chemistry

    Calculate the percent ionization of a .31 molar solution of acetic acid. The ionization constant of acetic acid is 1.8 x 10^-5

More Similar Questions