Question

On dissolving salt in water, salt splits into Na and Cl. As i was taught that Na instantly reacts with water and burns. Then why doesn’t Dissolved Na burn in water?

Answer 1

Hint: The chemical formula for sodium chloride is NaCl, which represents a 1:1 ratio of sodium and chloride ions. 100 g of NaCl comprises 39.34 g Na and 60.66 g Cl, with molar weights of 22.99 and 35.45 g/mol, respectively. The salt that is mainly responsible for the saltiness of seawater and the extracellular fluid of many multicellular organisms is sodium chloride. Table salt is frequently used as a condiment and food preservative in its edible form.

Complete answer:
Salt dissolves in water at the molecular level because of electrical charges and because both water and salt molecules are polar, having positive and negative charges on opposing sides of the molecule. Because the chloride ion is negatively charged and the sodium ion is positively charged, the bonds in salt compounds are referred to as ionic. In the same way, a water molecule is ionic in nature, but the connection is called covalent because two hydrogen atoms are positioned on one side of the oxygen atom, which has a negative charge.
When salt is combined with water, the salt dissolves because the water's covalent bonds are stronger than the salt molecules' ionic bonds. The negatively-charged chloride ions attract the positively-charged water molecules, while the positively-charged sodium ions attract the negatively-charged water molecules. In essence, a tug-of-war follows, with the water molecules emerging victorious. The ionic connection that held the sodium and chloride ions together is broken as water molecules pull them apart. This produces a homogenous solution.
A chemical transition occurs when sodium chloride is dissolved in water, resulting in a solution of sodium and chloride ions. Because of the polar nature of water, the sodium and chloride ions dissociate, making this solution an electrolyte (one that can conduct electricity).
 $NaCl\left(s\right)+H_{2}O\rightleftharpoons N{a}^{+}(aq)+C{l}^{-}(aq).$
When you put a piece of elemental sodium metal in water, it reacts quickly and aggressively. This is a chemical process in which sodium metal is oxidised to sodium cations, resulting in sodium hydroxide and hydrogen gas, both of which can ignite. The chemical equation that is balanced is:
 $2Na\left(s\right)+2H_{2}O(l)\to 2NaOH\left(aq\right)+H_2(g)$ .

Note:
The slightly electropositive sodium part of table salt is attracted to the slightly electronegative oxygen portion of water molecules when put in water. The slightly electronegative chlorine part of NaCl attracts the slightly electropositive hydrogen portion of water at the same time.
Although no real connection is formed in either scenario, the attractions cause a tug-of-war between the ionic bonds of NaCl and the covalent bonds of $H_{2}O$ .