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Spectrophotometry problem

  1. Sep 4, 2007 #1
    1. The problem statement, all variables and given/known data

    If a 0.390 mM solution of MnO41- has an absorbance of 0.585 at 525 nm in a 1.000 cm cell. What is the concentration of a MnO41- solution that has absorbance of 0.330 in the same cell at that wavelength?

    2. Relevant equations


    3. The attempt at a solution

    c(1) =concentration =.390 *10^-9 M
    wavelength = 525*10^-9 m
    pathlength = 1*10^-2 m
    A(1)= absorbance = .585
    A(2) = .330

    I think the wavelength and pathlength are irrelevant to finding the concentration of (MnO4)1-

    A(1)/A(2)= c(1)/c(2) => c(2)=c(1)*A(2)/A(1)

    C(2)= (.330) *(.390*10^-9)/(.585) = 2.20*10^-9
     
    Last edited: Sep 4, 2007
  2. jcsd
  3. Sep 4, 2007 #2

    symbolipoint

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    You have it; at least symbolically. Your constants substituted look good also.
    ...
    Now, how do you know that the concentration and absorbance are in a linear relationship (they probably are.)?
     
  4. Sep 5, 2007 #3

    chemisttree

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    It looks good except that a millimolar (mM) is 10^-3 moles/liter not 10^-9 moles/liter.
     
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