Question

Why is NaCl soluble in water?

Answer 1

Hint :Sodium chloride is an ionic compound with a high ionic strength. This is because the oppositely charged ions have a strong electrostatic attraction (cations and anions). When metals (in this case, sodium) react with non-metals, this is usually the case (in this case, chloride).

Complete Step By Step Answer:
Water is a polar molecule. It is, in fact, extremely polar. This means that a water molecule's partial positive and partial negative charges form polar bonds in an asymmetrical arrangement.
Water is made up of two hydrogen atoms and one oxygen atom. In $ {H_2}O $ , the atomic bonds are covalent, which means the electrons are shared. As a result, electrons closer to the oxygen atom have a negative charge, whereas electrons closer to the hydrogen atom have a positive charge.
NaCl, on the other hand, is made up of sodium ions that are positive and chloride ions that are negative. As a result, the water molecule's polar ends attract the oppositely charged parts of NaCl. To put it another way, positively charged water molecules attract negative chloride ions, while negatively charged water molecules attract positive sodium ions.
The positively charged sodium ions are attracted to the negative polar area of the water molecule, which is why salt dissolves in water. Similarly, negatively charged chloride ions are attracted to the water molecule's positive polar area. The attractive forces between the positive sodium ions and the negative chloride ions are overcome by the attractive forces with the water molecule, resulting in dissociation and the ionic compound NaCl entering solution.
 $ NaCl(s) + {H_2}O \to N{a^ + }(aq) + C{l^ - }(aq) + {H_2}O $ .

Note :
When NaCl dissolves in water (which requires heat energy), the strong ionic bonds are broken and the ions interact with the water molecules (releasing heat energy). In comparison to plain water and crystalline salt, the NaCl solution is much less orderly in water. Entropy increases whenever a solute dissolves in a solution.