A reaction mixture is in a 5.4 L flask at 25 oC initially contains only 7.64 grams of acetic acid. (CH3COOH). Set up your I.C.E. table and use it to answer the following questions. HINT: You will need to look up the Ka for this equilibrium reaction.
CH3COOH(aq) ¡ê CH3COO-(aq) + H+(aq)

a. How many moles of Acetic acid are in the solution at equilibrium?
b. What is the Kb for this reaction?
c. What is the pH of the equilibrium solution?
d. What is the pOH of the equilibrium solution?

  1. 👍 0
  2. 👎 0
  3. 👁 315
  1. I get tired of typing, CH3COOH we will call HAc. That is 7.64 g/molar mass HAc = 7.64/60 = 0.127 moles. You should do it more accurately than that since I estimated the molar mass of HAc.
    It ionizes as
    .................HAc -->H^+ + Ac^-

    Ka = (H^+)(Ac^-)/((HAc)

    a. See above.
    b. Did you make a typo here? If you mean Ka, look that up in your text or on-line. If you REALLY mean Kb, it is Kw/Ka.
    c. Substitute the ICE values into the Ka expression and solve for x. That will be moles H^+. Convert that to M by (H^+)= moles/L [Note: I must point out here that the problem does NOT tell you the volume of the solution. It tells you that the acetic acid is in a 5.4L flask BUT it doesn't say what else is there NOR its volume. I think the intent of the problem is that the flask CONTAINS 5.4 L of solution]. After moles H^+ are converted to M, then pH =-log(H^+).
    d. pH + pOH = pKw = 14. Solve for pOH.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Consider the generic reaction: 2 A(g)+ B(g)--> 2C(g). If a flask initially contains 1.0 atm of A and 1.0 atm of B, what will be the pressure in the flask if the reaction proceeds to completion? (Assume constant volume and

  2. Chemistry

    A 0.879 g sample of a CaCl2 ∙ 2 H2O / K2C2O4 ∙ H2O solid salt mixture is dissolved in 150 mL of deionized water. A precipitate forms which is then filtered and dried. The mass of this precipitate is 0.284 g. The limiting

  3. chemistry

    Consider the following reaction in a closed reaction flask. If 0.600 atm of gas A is allowed to react with 1.20 atm of gas B and the reaction goes to completion at constant temperature and volume, what is the total pressure in the

  4. Chemistry

    A 1.0 mL volume of 0.010 M H2SO4 is added to a mixture of 6 drops of 0.010 M HIO3, 14 drops of deionized water, and 1 drop of starch solution. A color change in the reaction mixture occurred after 56 seconds. a. Assuming 20 drops

  1. Chemsitry

    The equilibrium between three substances, a, B and c is shown below. A(g) + B(g) C(g) Initially there were 0.1 mol of a and 0.2 mol of B in the reaction mixture. a and B reacted together to produce an equilibrium mixture

  2. Chemistry help please!!!

    Experimental Procedure, Part F. A 1.0- mL volume of 0.010 M H2SO3 is added to a mixture of 12 drops of 0.01 M HIO3, 8 drops of deionized water, and 1 drop of starch solution. A color change in the reaction mixture occured in 40

  3. Science

    Why does the design of the vacuum flask minimize heat transfer by conduction? A)One flask is smaller than the other flask. B)One flask is more reflective than the other flask. C)There is no air between the two flask. D)The two

  4. Chemistry

    Consider the reaction: 2HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2H2O(l) ∆H = - 118 kJ Calculate the heat when 100.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.50 M Ba(OH)2. Assuming that the temperature of both solutions was

  1. chemistry

    50.0 mL of a solution of HCl is combined with 100.0 mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C and the final temperature after reaction is 31.2°C. What is the molarity of the HCl solution?

  2. chemistry

    A 100 L flask contains a mixture of methane and argon gasses at 25 degree C . The mass of argon present is 228 g and the mole fraction of methane in the mixture is 0.650 . calculate the total kinetic energy of gaseous mixture

  3. Chemistry

    If the initial concentration of is 0.250 , and the reaction mixture initially contains no products, what are the concentrations of and after 80 ?

  4. Chem

    I stuck on this problem. Can you help me to solve it? A reaction mixture in a 3.67L flask at a certain temp. initially contains 0.763g H2 and 96.9g I2. At equilibrium, the flask contains 90.4g HI. Calculate the equilibrium

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