chemistry

posted by .

A particular solution has a [H3O+] 2.44 x 10^-4. Therefore, the [OH-]=
4.10 x 10^3
4.10 x 10^-11
2.44 x 10^-4
1.71 x 10^-8
9.09 x 10^-16

  • chemistry -

    (H^+)(OH^-) = Kw = 1E-14

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Calculate the end point pH, when 25 mL of 0.01 mol/L HCl solution reacts exactly with 25 mL of 0.1 mol/L NH4OH solution. NH3 Kb = 1.8 x 10^-5 This will be the pH of NH4Cl solution. NH4+ + HOH ==> NH3 + H3O^+ Ka = Kw/Kb = (NH3)(H3O^+)/(NH4^+). …
  2. chemistry

    what is the pH of a solution that is .15 M in HOCl and .25 M NaOCl after .05 mol HCl/L has been bubbled into the solution?
  3. Help Chemistry

    Can you please tell me if these are right?
  4. Chem

    Please tell me if these are right! What are the [H3O+] and [OH-] for a solution with the following pH values?
  5. chemistry

    7). The pH of a solution is 2.89. What is the [H3O+]?
  6. chemistry

    The pH of an HCl solution is found to be 1.74. Therefore the [H3O+] is:
  7. Chemistry(Please respond, thank you)

    What is the [H3O+] for a neutral solution at 50 degrees celsius?
  8. chemistry

    1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the solution?
  9. Chemistry

    Calculate the pH of a solution in which a. [H3O+] = 7.8 x 10-7 M pH = b. [H3O+] = 5.1 x 10-6 M pH = c. [H3O+] = 6.1 x 10-5 M pH = d. [H3O+] = 9.3 x 10-4 M pH = I get 8.1 9.5 9.1 6.7 but its wrong please someone help!
  10. chemistry

    The pH of a 0.00100 M solution of a particular acid is 4.95 at 25°C. Use the solution pH to calculate the concentration of hydronium ion present [H3O+]

More Similar Questions