chemistry

posted by .

Calculate [acetate] of 0.057 mol/L solution of acetic acid of Ka = 1.76x10^-5

i know to find Ka it's:
Ka= products/reactants
so i tried doing an ICE table with the equation to be:
CH3CO2 + H2O <--> CH3COOH + H
am i on the right track? if not...help please!

  • chemistry -

    Yes, you just stopped too soon.
    Let's call acetic acid HAc.
    HAc --> H^+ + Ac^-

    Then, as you have it, Ka = (H^+)(Ac^-)/(HAc) = 1.76 x 10^-5.

    Now you do the ICE chart.
    (H^+) is x
    (Ac^-) is x
    (HAc) is 0.057 -x

    I will leave the equation for you to solve. Please note, however, that while the x in 0.057-x USUALLT can be neglected, I don't think it can in this problem and you will need to solve the quadratic equation (or do it by successive approximations). The only real difference between this problem and most of the others like this one is that this one asks for Ac^- (instead of asking for pH etc) and all you need to do is to realize that acetate and H^+ are the same.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chem

    The equilibrium constant Kc equals 5.90 for the reaction CH3COOH + C2H5OH <==> CH3COOC2H5 + H2O Find the molar concentrations of acetic acid, ethanol, ethyl acetate, and water at equilibrium when .10 M acetic acid and .20 M ethanol …
  2. chemistry-

    How do I construct an ICE table for this question. CH3COOH + NaOH --> CH3COONa + H2O Fill in the equilibrium line of the table. [Think about the initial pH and think about the pH at the end point of the titration. Initial pH 2.72 …
  3. Chemistry

    You are carrying out the titration of 100.0 mL of 1.000M acetic acid with 1.000 M sodium hydroxide. Ka = 1.76x10^-5 of acetic acid. (a) Calculate the initial pH of your acetic acid sample. (b) Calculate the pH of the solution after …
  4. chemistry

    hi, i am trying to develop a lab where i find the solubility of Sodium acetate. I was wondering in i was in the right path. We are given these three compounds: Acetic acid aka vinegar baking soda (sodium hydrogen carbonate) 0.100mol/l …
  5. Chemistry 102

    For a question like “calculate the pH of an aq.solution that is 1.0 M CH3COOH and 1.0 M CH3COONa, how do you know to write the equation like this: CH3COOH + H2O => H3O+ + CH3COO- and not like H3O+ + CH3COO- => CH3COOH + H2O …
  6. Chemistry

    Complete and balance the following neutralization reactions. then, write the names of all the reactants and all the products in each chemical reaction. A) HNO3 + Al(OH)3 = 3HNO3 + Al(OH)3 -> Al(NO3)3 + 3H2O Reactants: Nitric acid, …
  7. school

    What is the pH of 0.1 M formic acid solution?
  8. science

    Calculate the pH of a solution of ammonium acetate (CH3COONH4) 0,85M knowing that for NH3 Kb = 1,79x10-5 and CH3COOH Ka = 1,76x10-5 and commented on the result obtained. Then calculate the percentage of acetic acid product at equilibrium
  9. Chemistry

    A solution of acetic acid, 1.0 mol L–1 CH3COOH, contains sodium acetate, NaCH3COO. The percent ionization of the above solution is 0.25%. The Ka for acetic acid is 1.8 x 10–5. Which of the following is the concentration of NaCH3COO …
  10. Chemistry

    I Just don't know what to do, I think I understand, but im not sure because all of the compounds are liquid. I would know how to do it if they were aqueous, and just the water is liquid, but they are all liquid. Determine the acid …

More Similar Questions