chemistry

A weak base with a concentration of 1.3 mol/L has a percent ionization of 0.72%. What is the Kb of this weak base?

could someone help me with this question or how to get started?

  1. 👍
  2. 👎
  3. 👁
  1. Call the weak base BOH.
    BOH <==> B^+ + OH^-

    Kb = (B^+)(OH^-)/(BOH)

    If 0.72% ionized, that means(H^+) must be 1.3 M x 0.0072 = ??
    Of course (OH^-) must be the same.
    If BOH is 0.72% ionized, it must be 100% - 0.72% unionized.
    Substitute into Kb expression and solve for Kb. Post your work if you get stuck.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    write the balanced equation for the ionization of the weak base pyridine, C5H5N, in water

  2. Chemistry

    Select the statements that correctly describe buffers.? 1) The pH of a buffer solution does not change significantly when any amount of a strong acid is added. 2) The Ka of a buffer does not change when any amount of an acid is

  3. chemistry

    Strong base is dissolved in 665 mL of 0.400 M weak acid (Ka = 3.69 × 10-5) to make a buffer with a pH of 3.94. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) -> H2O(l) + A-(aq) Calculate the pKa

  4. Chemistry

    What will happen if a small amount of hydrochloric acid is added to a 0.1 M solution of HF? A) The percent ionization of HF will increase. B) The percent ionization of HF will decrease. C) The percent ionization of HF will remain

  1. Chemistry 2 - Acids and Bases

    Hydrazine (NH2NH2) is a weak base that ionizes in water as follows. NH2NH2(aq) + H2O(l) HNH2NH2^+(aq) + OH^−(aq) Calculate the concentration of OH^− ions in a 0.20 M solution of hydrazine, given that the base-dissociation

  2. Chemistry

    Which of the following statements are true about a strong base and a weak base at a pH of 11? A) HCl will not bring the pH of either solution to pH 7. B) Both bases require the same amount of HCl to reach pH 7 because they are

  3. Chemistry

    Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid

  4. Chemistry

    The Ka of a monoprotic weak acid is 3.29 × 10-3. What is the percent ionization of a 0.176 M solution of this acid?

  1. Acid-Base chem

    Which of the following would for a buffer if added to 250.0 mL of .150 M SnF2? a).100 mol HCl b).060 mol HCl c).040 mol HCl d).040 mol NaOH e).040 mol HF I figured I could find out the pH of the solution with HCl/NaOH/HF added,

  2. AP Chemistry

    (a) What is the pH of a 2.0 molar solution of acetic acid. Ka of acetic acid = 1.8 x 10¯5 (b) A buffer solution is prepared by adding 0.10 liter of 2.0 molar acetic acid solution to 0.1 liter of a 1.0 molar sodium hydroxide

  3. Chemistry

    Calulate the degree of ionization for NH3(aq) in 1.0 M solution, Kb = 3.236E-4. I've seen degree ionization for acids and not bases. Do I need to find the Ka [H+] value of the base to determine the degree of ionization?

  4. AP Chemistry

    A given weak acid HZ has a Ka=1.7×10−6. What is the H3O+ concentration of a solution of HZ that has a concentration of 0.78 mol/L? What is the pH of this solution of HZ? What is the percent ionization of HZ in this solution?

You can view more similar questions or ask a new question.