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Slim24/7
Lv 5
Slim24/7 asked in Science & MathematicsChemistry · 6 years ago

What is the [OH-], [H+], and pH of a 0.11 M KOH solution?

Assuming complete ionization, how do I find the [OH-], [H+], and pH of a 0.11 M KOH solution?

Please help! Test tomorrow!

2 Answers

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  • hcbiochem
    Lv 7
    6 years ago
    Favorite Answer

    Since ionization is complete, [OH-] = 0.11 M because KOH ionizes into K+(aq) and OH-(aq).

    Now, in any aqueous solution, [H+] X [OH-] = Kw = 1.00X10^-14. So,

    [H+] X 0.11 = 1.0X10^-14

    [H+] = 9.1X10^-14 M

    pH = -log [H+] = 13.04

  • Jan
    Lv 7
    6 years ago

    pH=13.04

    H^+=10^-13.04 M

    OH^- = 0.11

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