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Analytical Chemistry

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The question:

The pH of a solution is defined as
pH = -log[H3O+].
If the pH of a solution is 3.72(+/- 0.03), what is the [H3O+] and its absolute standard deviation?

Answer: How would I carry this out? I know to find the hydronium concentration wouldn't i just take e^3.72? How do I do it the way they are asking for?

  • Analytical Chemistry - ,

    H3O+= e^-pH+-error
    = e^-pH * e^-+error
    =e^-3.72 * e^+-.03

  • Analytical Chemistry - ,

    pH = -log(H3O^+)
    3.72(+/-0.03) = -log(H3O^+)
    So the answer is antilog -3.72 (+/- ?) = 0.0001905 +/- ?.
    The formula for handling antilogs (10^-pH) is (s/y)= 2.303 x (abs std dev) = (s/y) = 2.303 x (0.03)
    (s/y) = 0.0691
    s = 0.0691 x 0.0001905 = 0.000013
    answer is
    0.0001905 +/-0.000013 which I would round to 0.00019 +/-0.00001
    Check my work, especially for typos

  • Analytical Chemistry - ,

    I believe (H3O^+) = 10^-pH

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