Chemistry

posted by .

A weak acid solution, HX 0.37 M, has a pH of 3.70. Calculate the acidity constant for this acid.

  • Chemistry -

    pH = -log(H^+)
    3.70 = -log(H^+)
    Convert that; I get about 2E=4 but you need to confirm that.
    ...........HX ==> H^+ + X^-
    I.........0.37....0......0
    C........-2E-4...2E-4...2E-4
    E......0.37-2E-4..2E-4...2E-4

    Substitute into the Ka expression and solve for Ka.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89?
  2. chemistry

    Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?
  3. chemistry

    Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?
  4. Chemistry

    Given acidity constant,Ka of benzoic acid is 6.28 X 10^-5. pH of 0.15 molar solution of this acid is ?
  5. 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 …
  6. AP Chemsitry

    A solution of an unknown monoprotic weak acid was titrated with 0.100 M NaOH. The equivalence point was reached when 37.48 ML of base had been added. From a second buret, exactly 18.74 of 0.100 M HCl were added to the titration solution. …
  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 help

    A 15.00 mL sample of an unknown monoprotic weak acid solution is titrated with 0.35 M NaOH. The initial buret reading is 0.23 mL. The phenolphthalein indicator turns the solution light pink when the buret reads 29.58 mL. B. How many …
  10. Chemistry

    An unknown monoprotic acid has a pH of 2.87. Is this acid weak or strong if 22.32 mL of 0.112 M NaOH is required to titrate 25.00 mL of the acid?

More Similar Questions