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chemistry

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enough of a monoprotic acid is dissolved in water to produce a 0.0111M solution. The pH of the resulting solution is 2.62. Calculate the Ka for the acid.

  • chemistry -

    pH = 2.62 = -log (H^+); therefore,
    (H^+) 0.0024
    ............HA ==> H^+ + A^-
    I........0.0111.....0.....0
    C.........-x........x......x
    E.......0.0111-x....x......x
    x = 0.0024
    Ka = (H^+)(A^-)/(HA)
    (H^+) = 0.0024 = (A^-)
    (HA) = 0.0111-0.0024 = ?
    Substitute and solve for Ka.

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