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11 March, 12:27

What are the concentrations of H3O + and OH-? in oranges that have a pH of 3.69?

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  1. 11 March, 12:40
    0
    pH = - log [H3O+]

    [H3O+] = 1x10-3.71 = 1.95x10-4 M

    You should be able to find [OH-] recalling that Kw = [H3O+][OH-] = 1x10-14
  2. 11 March, 12:50
    0
    [H+] = 2.04 * 10^-4 M

    [OH-] = 4.90*10^-11 M

    Explanation:

    Step 1: Data given

    pH = 3.69

    Step 2: Calculate [H3O+]

    pH = 3.69 = - log [H+] = - log [H3O+]

    [H+] = [H3O+] = 10^-3.69 = 2.04 * 10^-4 M

    Step 3: Calculate pOH

    pH + pOH = 14

    pOH = 14 - 3.69 = 10.31

    Step 4: Calculate [OH-]

    pOH = 10.31 = - log [OH-]

    [OH-] = 10^-10.31 = 4.90*10^-11 M
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