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Ionic exchange

  1. Feb 19, 2013 #1
    1. The problem statement, all variables and given/known data

    10 mL solution of 0.5 M CrCl(OH2)52+ is allowed to aquate to Cr(OH2)63+. To determine an approximate rate of reaction, the amounts of CrCl(OH2)52+ and Cr(OH2)63+ present after a certain period of time are evaluated. This is done by pouring the solution on a cation exchange resin in the H+ form and then titrating the displaced H+ with base. If 80 mL of 0.15 M NaOH is required to neutralize the liberated H +, what was the concentration of CrCl(OH2)52+ and Cr(OH2)63+ in the solution?

    2. Relevant equations

    3. The attempt at a solution

    CrCl)OH2)5 +2

    V=10ml c=0.5M


    V=80mL c=0.15M

    Total volume=90mL

    im not really sure if im doing this right, any help please :(
  2. jcsd
  3. Feb 20, 2013 #2


    User Avatar

    Staff: Mentor

    I don't think you are doing it right, even if you have not wrote what you are doing and what c1 and c2 are.

    How many moles of H+ are liberated per each mole of CrCl(H2O)52+?

    How many moles of H+ are liberated per each mole of Cr(H2O)63+?

    If a mixture contains n1 moles of CrCl(H2O)52+ and n2 moles of Cr(H2O)63+, how many moles of H+ will be liberated? How many moles of NaOH will be needed to titrate the elute?

    And finally, what does n1+n2 equal to?

    This gives you two equations in two unknowns and finding the concentrations of both complexes shouldn't be difficult.
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