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!