Ask Question
31 March, 19:53

Calculate the pH of a solution formed by mixing 300.0 mL of 0.30 MHClO with 150.0 mL of 0.20 MLiClO. The Ka for HClO is 2.9*10-8.

+3
Answers (1)
  1. 31 March, 21:02
    0
    pH = 7.06

    Explanation:

    The solution formed will be a buffer solution, which is a solution that contains a weak acid-base conjugate pair. The Henderson-Hasselbalch equation may be used to calculate the pH of a buffer solution, where A⁻ is the conjugate base (in this case, ClO⁻) and HA is the conjugate acid (in this case, HClO):

    pH = pKa + log ([A⁻]/[HA]) = - log (Ka) + log ([A⁻]/[HA])

    The concentration of the ClO⁻ in the final solution can be calculated using the dilution equation. The volume of the final solution is 450.0 mL.

    C₂ = (C₁V₁) / V₂ = (0.20M) (150.0mL) / 450.0mL = 0.066 ... M

    Similarly, the concentration of HClO in the final solution is:

    C₂ = (C₁V₁) / V₂ = (0.30M) (300.0mL) / 450.0mL = 0.20 M

    Substituting these values into the Henderson-Hasselbalch equation gives:

    pH = - log (Ka) + log ([A⁻]/[HA]) = - log (2.9 x 10⁻⁸) + log (0.066 ... / 0.2) = 7.06
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “Calculate the pH of a solution formed by mixing 300.0 mL of 0.30 MHClO with 150.0 mL of 0.20 MLiClO. The Ka for HClO is 2.9*10-8. ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers