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In a .25 M solution, a weak acid is 3.0% dissociated.

A. calculate the pH of the solution
B. calculate the Ka of the acid

Please explain steps.

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2 answers
  1. ..............HA ==>H^+ + A^-
    initial....0.25M....0......0
    change.......-x......x......x
    equil......0.25-x....x.....x
    If it is 3% dissociated, that means that x = 0.25*0.03 = ?
    Substitute into the Ka expression and solve for Ka.
    pH = -log(H^+)

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  2. Please help me solved this problem

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