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PH problem

  1. Nov 26, 2007 #1
    1. The problem statement, all variables and given/known data
    Calculate the pH of a solution of a concentration of 0.23 mol/L of H2SO4, if it completely ionizes in the solution.

    2. Relevant equations
    [H3O] = 10[tex]^{-pH}[/tex]
    pH = -log[H3O]

    3. The attempt at a solution
    The answer I got for this question is 0.34. I got this answer by first writing out the ionization equation for H2SO4, and determining how many hydronium ions are made, which I got as two. Then, I found out the concentration of the hydronium ions by multiplying 0.23 mol/L by 2. Then, I used pH = -log[H3O], and got the answer of 0.34. Am I right?
  2. jcsd
  3. Nov 26, 2007 #2


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    Gold Member

    Your described method is good. You are looking for the negative logarithm of 0.46 Molar.
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