Chemistry

posted by .

What are some of the equilibrium expressions that chemists use for weak acid equilibrium?

  • Chemistry -

    Ka = (products)/(reactants)
    with coefficients becoming exponents.

  • Chemistry -

    Are there any more expressions for weak acids equilibrium? It would be helpful in the long run to know what they all are if there are any more.

  • Chemistry -

    You're question is so general that I didn't know what to write the first time and certainly I don't know what to write now. For a weak acid, such as HA, it ionizes as
    HA(aq) + H2O(l) ==> H3O^+(aq) + A^-(aq) in which aq stands for aqueous (as in solution) and l stands for liquid (meaning pure H2O), the
    Ka = (H3O^+)(A^-)/(HA)
    All follow that same generic Ka. There are some diprotic and triprotic acids but they follow the same rules. For example, H2CO3 is
    H2CO3(aq) + H2O(l) ==>H3O^+(aq) + HCO3^-(aq) and k1 for that ionization is
    k1 = (H3O^+)(HCO3^-)/(H2CO3)

    The second hydrogen then ionizes as
    HCO3^-(aq) + H2O(l) ==>H3O^+(aq) + CO3^2-(aq) for which k2 is
    k2 = (H3O^+)(CO3^2-)/(HCO3^-)
    etc.

    H3PO4, a triprotic acid, works the same way and it has a k1, a k2, and a k3 in which one H comes off at a time.
    If you have a specific problem it would be easier to answer that than trying to stay with general cases.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. ap chem

    A 9.00 M solution of a weak acid, HA, has a pH of 1.30 1.) calculate [A-] at equilibrium 2.) calculate [HA] at equilibrium Use pH to get (H^+). Ka = (H^+)(A^-)/(HA) (A^-) = (H^+). (HA) = 9 Plug and chug. Post your work if you get stuck.
  2. chemistry

    Lactic acid, HC3H5O3(aq) is a weak acid that gives yougurt its sour taste(Yeeeeecccckkk). Calculate the pH of a 0.0010 mol/L solution of Lactic acid. The Ka for lactic acid is 1.4 x 10^-4 For Further Reading chemistry - DrBob222, Saturday, …
  3. chemistry

    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 …
  4. Chemistry

    The pH of a weak monoprotic acid, HA, is 4.55. It took 39.22 ml of 0.2334 M NaOH to titrate 25.00 ml of the acid. a. Write an equation for the above reaction. b. Calculate the molarity of the weak acid c. Write the equilibrium equation. …
  5. CHEMISTRY HELP!!

    Formic acid (HCHO2) is a component of bee stings. It is a weak acid and dissociates according to the equilibrium shown below: HCHO2 <===> H+ + CHO2- Kc = 1.8 x 10-4 For a 0.5 M solution of formic acid, we wish to determine the …
  6. Chemistry

    In the titration of a weak acid with a strong base, the pH at the equivalence point is affected mostly by a.hydrolysis (reaction with water) of the weak acid b.the dissociation of water molecules c.the presence of excess base d.the …
  7. Chemistry

    Consider 2 separate solutions, one of a weak acid HA and one of HCL. Assume that you started with 10 molecules of each. Draw a picture of what each solution looks like at equilibrium. Ok to my very limited knowledge on this subject …
  8. Chemistry

    What are some equilibrium expressions that chemists use for weak acid equilibrium?
  9. Chemistry

    What are some equilibrium expressions that chemists use for weak acid equilibrium?
  10. Chemistry

    Ka for a weak acid HA = 3.46x10^-8, calculate K for the reaction of HA with OH- HA + OH- = A- + H2O This is an equilibrium question, but I do not understand how to find the equilibrium constant K, from the equilibrium constant of an …

More Similar Questions