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Weak base/ Strong acid pH

  1. Mar 14, 2007 #1
    Question: TRIS is a weak base. Compute pH of a solution containing .050 moles of TRIS and .020 moles of HCl in a total volume of 2L. pKb for TRIS is 5.92. Use RNH2 to represent TRIS.

    Equation: pH = pKa+ log ([conjugate base]/[acid])

    change equation for pOH:
    pH = 14-pOH
    pOH = pKb + log ([conjugate acid]/[base])
    pOH = 5.02 + log (.010/.025) <---- I converted to mol/L for these values
    pOH = 5.52
    pH = 8.48

    Real Answer: 8.26

    Can someone show me where I went wrong? Thanks!
  2. jcsd
  3. Mar 14, 2007 #2


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    Staff: Mentor

    What are your conjugated acid and base? What is your base concentration? (Hint: write reaction equation).

    Last edited by a moderator: Aug 13, 2013
  4. Mar 14, 2007 #3
    They don't say what the conjugate acid and base is, except that the base is RNH2, so then its conjugate acid would be RNH3, right?

    The base concentration would be .05/2 = .025 M.

    The reaction equation would be
    RNH2 + HCl <--> H2O + RNH3
    .25M .1M 0
    -.1M -.1M .1M
    .15M 0M .1M

    pOH = pKb + log (.1/.15)
    pOH = 5.92 + log (.1/.15)
    pOH = 5.74
    pH = 8.26


    That's it! Thank you! :D :D
  5. Mar 31, 2009 #4
    Why is it better to use a weak base(such as calcium carbonate) to neutralise strong acid (such as hcl) rather than strong base?

    Thank you so much
  6. Mar 31, 2009 #5


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    Homework Helper
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    Gold Member

    Generally, a weak base is not better and not worse. The choice depends on the application. Why do you ask?

    If you use calcium carbonate to neutralize a strong acid, you hopefully are not worried about the presence of calcium, and the resulting carbon dioxide may be mostly insoluble, but beware of bubbling or foaming. Depending on quantities involved of the base(calcium carbonate) and the acid, you might be choosing to produce a buffer; is that what you wanted? Did you want some bicarbonate present?
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