Chemistry

posted by .

Calculate the pH of a solution at 25.0 °C that contains 1.94 × 10-10 M hydronium ions.

  • Chemistry -

    I would convert 1.94E-10 to pOH.
    pOH = -log(OH^-), then
    pH + pOH = pKw = 14.
    You know pOH and pKw, solve for pH.

    If you prefer you can do it this way(H^+)(OH^-) = Kw = 1E-14
    You have OH^-, solve for (H^+), then
    pH = -log(H^+)

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    What is meant by the hyrdration of the hydrogen ion?
  2. CHEM

    A concentrated weak acid is best described as which of the following?
  3. Chem I

    Calculate the concentrations of hydronium and hydroxide ions in a solution prepared by dissolving 0.345g of solid NaOH in enough water to make 225mL of solution. Also calculate the pH and pOH of the solution.
  4. chemistry

    which solution has the highest concentration of hydroxide ions?
  5. Science

    You have a solution that contains Ag* ions and another that contains Na* ions. How would adding a solution that contains Cl- ions to these solutions enable you to tell which is which?
  6. chemistry

    calculate the hydronium ion concentration in an aqueous solution that contains 2.50x10^-6M in hydroxide solution
  7. Science

    5. You have made the following two solutions: X) hydrogen ion concentration = 1 x 10-5M Y) pH = 4 State which statements below are true and which are false: a. Solution X contains 1 x 10-9M hydroxide ions. b. Solution X contains more …
  8. Chemistry

    Calculate the pH of a solution at 25.0 °C that contains 1.94 × 10-10 M hydronium ions.
  9. Physics

    You have a solution that contains Ca2+ ions and another that contains Na+ ions. How would adding a solution that contains CO2-3 ions enable you to tell which is which?
  10. Chemistry

    Calculate the pH of a 0.18 M solution of cyanide ion, CN- given the Ka (HCN) = 6.2 x 10^-10. I know how to calculate Ka and Kb values no problem, but I don't know which value to use in my calculations. Is it based on the conjugate …

More Similar Questions