Chemistry

posted by .

A 0.10 M solution of a weak acid has a pH of 3.5 at 25%C. What is the equilibrium constant, Ka, for this acid?

  • Chemistry -

    What is 25%C?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    A 0.010 M solution of a weak monoprotic acid is 3.0% dissociated. What is the equilibrium constant, Ka, for this acid?
  2. chemistry

    A 0.010 M solution of a weak monoprotic acid has a pH of 3.70. What is the acid-ionization constant, Ka, for this acid?
  3. Chemistry

    0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 5.0 * 10^-4 M. What is the equilibrium constant, Ka, for this acid?
  4. Hayden

    Chloroacetic acid has a relatively large equilibrium constant, so at low acid concentrations it is necessary to use the quadratic equation in order to calculate the concentrations of the aqueous species. Ka for ClCH2COOH is 1.4 ยด …
  5. 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. …
  6. chemistry

    2- A 0.310 M solution of a weak acid, HX, has a pH of 2.53 a. Find the [H+] and the percent ionization of nitrous acid in this solution. b. Write the equilibrium expression and calculate the value of Ka for the weak acid. c. Calculate …
  7. Chemistry-Dr Bob help!!

    0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid?
  8. Chemistry

    1 g of acid was mixed with 120 ml of distilled water and the solution was filtered into a clean dry beaker. A 25 ml aliquot of this solution was titrated with 0.1120 M NaOH. The pH of the acid was recorded to be 4.42. Calculate the …
  9. Chemistry

    A solution of a weak acid (.025M, 200ml) is mixed with a solution of NaOH ( 0.015M, 150ml). The equilibrium pH is 5.51. What is the Ka of the weak acid?
  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