In case of solvation , Who converts gaseous ions to aqueous ? Why do we even have gaseous but not solid ions?

Question

We take Nacl and dissolve it in water. There is formation of $Na^+$ and $Cl^-$ gaseous ions along with 2H⁺ and $Cl^{2-}$ aqueous ions.

Then , Na⁺ is attracted towards $Cl^{2-}$ and 2H⁺ is attracted towards $Cl^-$ ions.

Energy required by water molecules to separate the NaCl molecules is knows as Lattice enthalpy.

Energy required to form aqueous NaCl molecule is called hydration enthalpy.

My questions are:

1. Who is the one that converts gaseous ions of NaCl to aqueous ions?

2. During the dissolution of NaCl, why is there no formation of solid ions first but directly, it states that gaseous ions of NaCl are formed?

Also

Answer 1

We define reactions uniquely depending on the reactants and products. Here are examples related to your question.

Formation: Na(s) + (1/2)Cl$_2$(g) $\rightarrow$ NaCl(s)

Lattice Formation: Na$^+$(g) + Cl$^-$(g) $\rightarrow$ NaCl(s)

Solution: NaCl(s) $\rightarrow$ NaCl(aq)

Hydration: Na$^+$(g) $\rightarrow$ Na$^+$(aq)

Atomization: Na(s) $\rightarrow$ Na(g)

A significant observation here is that the STATE of the reactants and products is also required because it is a unique identifier.

As to your questions ...

1. Who is the one that converts ...

We can convert NaCl(s) to gaseous ions experimentally through processes that may involve multiple steps, including vaporization and ionization.

2. During the dissolution of NaCl(s), why is there no formation of solid ions first but directly, it states that gaseous ions of NaCl are formed?

The experimental dissolution of NaCl(s) does not involve formation of gaseous ions. It involves formation and solvation of aqueous ions. The two steps (dissolution and solvation) are often not easily separated.

What you refer to is the case where we imagine the dissolution of NaCl(s) happening through a set of steps that include the formation of gaseous ions. The process to combine reaction steps that go from a given set of reactants to a given set of products is formalized in what is called a Born-Haber cycle. This example demonstrates how some of the above reactions fit into a Born-Haber cycle diagram for NaCl(s).

Just because we imagine a reaction path on the Born-Haber cycle does not mean that the reaction occurs experimentally. Indeed, one power to the Born-Haber cycle is to back-calculate an energy for a reaction that does not occur experimentally but that has significant theoretical utility as a building block to obtain other values.