# Is common salt soluble in all types of water?

$N a C l \left(s\right) r i g h t \le f t h a r p \infty n s N {a}^{+} \left(a q\right) + C {l}^{-} \left(a q\right)$
When we write $N {a}^{+} \left(a q\right)$ we means the aquated sodium ion; this results from the chemical dissolution of salt in a water (i.e. aqueous) solvent. Another way of representing this would be: ${\left[N a {\left(O {H}_{2}\right)}_{6}\right]}^{+}$. The reaction above is a reversible chemical equilibrium, and on standing the salt would deposit as $N a C l$ crystals.
It is worthwhile at home to grow macroscopic crystals of salt. Take a saturated solution (a solution that is in equilibrium with undissolved salt), filter it, and add (precisely) 1 tiny crystal of salt. If evaporation is kept to a minimum (by covering the solution), aqueous salt will precipitate only on the 1 salt crystal that you added. I have grown very large crystals ($2.5 \times 2.5$ $c m$) of salt this way.