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March 28, 2017

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A tank contains exactly 10^(6)liters of pure water. 1.0*10^(-6) moles of HCl (g) is bubbled into this tank. What is the resulting pH?

The answer is 7, but I was only able to deduce that based on the fact that water has a neutral pH, but there's a mathematical way to do it and I'm not sure how to go about it.

  • Chemistry - ,

    I don't know.

  • Chemistry - ,

    HCl is a strong acid meaning that it dissociates 100%; therefore, 1E-6 mol/1E6L = 1E-12M HCl.
    HCl ==> H^ + Cl^-
    1E-12...0.....0
    -1E-12..1E-12..1E-12

    ..........HOH ==> H^+ + OH^-
    I...............1E-12....0
    C..................x......x
    E..............1E-12+x....x

    (H^+)(OH^-) = Kw = 1E-14
    (1E-12+x)(x) = 1E-14
    Solve the quadratic. I get all of these numbers on the calculator like
    9.99995E-8
    pH = -log(H^+) = 7.00000.
    With no temperature listed I couldn't look up the correct value for Kw at that particular temperature but I think this will do the trick.

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