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    Checking my work on one pH (and pOH) problem.

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    A solution in water has 1.0x10E-5 moles of H+ ion in 10.0 liters of solution.
    -What is the pH?
    -What is the concentration of the OH- ion?

    My notes give an example of:
    3.75 x 10E-4 with the result of -3.425968732

    However, when I attempt to run the example through my calculator I end up with 0.60205999...

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    Solution Preview

    Since pH = -log[H+] and you have 1x10E-5 moles in 10 L of solution,
    your [H+] = (1x10E-5 moles)/10L = 1x10E-6 molar (M),
    and therefore your pH = 6.0.

    Since Kw = 1x10E-14 = [H+]*[OH-],
    your [OH-] = (1x10E-14)/(1x10E-6) = 1x10E-8 M

    We can check this since pH + pOH = 14, and the negative log of the [OH-] = 8, so it's right.

    I don't know if ...

    Solution Summary

    Given a certain volume of H+ ions in solution, calculate the pH and [OH-]. The answer is fully explained.