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Composition of a Mixture by Acid-Base Titration

  1. Oct 4, 2007 #1
    A 1.00-g solid sample containing a mixture of table salt (NaCl) and citric acid (H3C6H5O7, a triprotic acid) is dissolved in 15 mL of water.
    Titration of the acid solution requires 40.00 mL of 0.2003 M NaOH solution to reach the endpoint.
    Calculate the mass percent H3C6H5O7 in the solid mixture.


    Can somone plz explain how to do this problem...??
     
  2. jcsd
  3. Oct 4, 2007 #2

    chemisttree

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    Start by writing out the neutralization equation.
     
  4. Oct 4, 2007 #3
    I have tried but i dont know how to solve for M2

    M1 x V1 = M2 x V2

    can u help plz
     
  5. Oct 5, 2007 #4

    chemisttree

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    Start by writing out the neutralization equation.
     
  6. Oct 5, 2007 #5
    First, figure out how many moles of NaOH were used, this will be equivalent to the amount of [tex]OH^{-}[/tex] in the titration mixture, if its the end point [tex]OH^{-} = H^{+}[/tex], I hope that gets you closer to your final goal, as its bad policy for us to just give you a full answer.

    Or, just do what chem said, write the neutralization equation (I do the more manual way personally ¬_¬ )
     
  7. Oct 5, 2007 #6

    symbolipoint

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    "triprotic acid".......... Which endpoint? Is your course "elementary chemistry" or is it undergraduate "Quantitative Chemistry"?
     
  8. Oct 5, 2007 #7
    I think he will be reffering to the third endpoint, rather than the first.
     
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