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Preetha

  • 2 years ago

10.0 ml of a 0.1 M solution of a metal ion solution of a Metal ion M2+ is mixed with a 10.0 ml Solution of a 0.1 M substance L. The following equation is established: M2+(aq)+2L(aq)<->ML2 2+(aq). At equilibrium the concentration of L is 0.01M. What is the equilibrium concentration of [ML2]2+? Please help me understand what I am doing wrong.

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  1. Preetha
    • 2 years ago
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    Hi Diva

  2. Preetha
    • 2 years ago
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    Diya

  3. Diyadiya
    • 2 years ago
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    Hi Ma'am :) But sorry i learnt about equlibrium last year ,i completely forgot

  4. Diyadiya
    • 2 years ago
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    I Hope someone will help you out soon =)

  5. Hershey_Kisses
    • 2 years ago
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    i know how to solve 10.0 mL of a 0.100 M it's comes out like this, Hope fully this can give you a little start : Change everything to moles. Multiply Molarity by Volume to get moles. First change L in moles. You can figure out how many moles of each are in equilibrium. If L = x moles, M2+ = x moles, ML2 = 3x moles. PS. To find L moles multiply the final concentration (given above) by the total volume, 200mL. Divide the moles by the total volume to get the concentration.

  6. Preetha
    • 2 years ago
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    That is a good start. I will redo the calculations.

  7. Hershey_Kisses
    • 2 years ago
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    That's good that you have a start :) !

  8. Preetha
    • 2 years ago
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    Thanks for trying Hershey. The important point that I got from you is that I have to redo the calculations with the new volumes.

  9. Rogue
    • 2 years ago
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    If I did it correctly, the answer should've been [M2+] = 0.04 M.

  10. Preetha
    • 2 years ago
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    That is what my nephew got, but the teacher says otherwise. Thanks Rogue!

  11. Rogue
    • 2 years ago
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    Alright, no problem :)

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