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Is this the correct explanation? (phase equilibria)

  1. Jan 17, 2016 #1

    TT0

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    1. The problem statement, all variables and given/known data
    Given the following reaction that has reached equilibrium: NaCl(s)←→NaCl(aq).
    For the phase equilibrium to exist, the NaCl(aq) must be a solution that is

    A. concentrated
    B. saturated
    C. dilute
    D. heated
    E. unsaturated

    2. Relevant equations
    -

    3. The attempt at a solution
    I chose B. My explanation is that the scenario is a block of salt is put into a beaker of water. The equilibrium exists when the solution is saturated so the remaining block cannot dissolve anymore and will stay solid. Is this the correct explanation? I am making sure because I have never seen a question like this before. Thank you very much!
     
  2. jcsd
  3. Jan 17, 2016 #2

    TT0

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    I am sorry about the misleading topic of the thread, I typed the wrong thing in.

    *Ignore this, I just saw how to edit the title.
     
  4. Jan 17, 2016 #3

    Borek

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    Staff: Mentor

    Yes, B it is. If the solution is not saturated, solid NaCl can't exist in the equilibrium with the solution - it will dissolve (until solution saturates).
     
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