Is this the correct explanation? (phase equilibria)

[TT0]

Homework Statement

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

Homework Equations

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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!

 

[TT0]

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.

 

[Borek]

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).