Ask Question
15 January, 02:09

A 0.22 M solution of a weak acid HA dissociates such that 99.5% of the weak acid remains intact (i. e., remains as HA). To the nearest hundredths, what is the pH of the solution?

+3
Answers (1)
  1. 15 January, 02:14
    0
    pH = 0.65975

    Explanation:

    HA ↔ A - + H + pH = - Log [H+] %α = ([A-] / [A-] + [HA]) * 100

    ∴ C HA = 0.22 M

    mass balance:

    ⇒ C HA = [A-] + [HA] = 0.22 M

    charge balance:

    ⇒ [H+] = [A-] ... [OH-] is neglected, is come frome the water.

    replacing in %α:

    ∴ %α = 99.5%

    ⇒ 99.5% = ([A-] / [A-] + [HA]) * 100

    ⇒ 0.995 = [A-] / 0.22 M

    ⇒ [A-] = (0.22 M) * (0.995) = 0.2189 M

    ∴ [A-] = [H+] = 0.2189 M

    ⇒ pH = - Log (0.2189)

    ⇒ pH = 0.65975
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “A 0.22 M solution of a weak acid HA dissociates such that 99.5% of the weak acid remains intact (i. e., remains as HA). To the nearest ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers