Question

Why is the NaCl boiling point high?

Answer 1

Hint: A substance's boiling point is the temperature at which the vapour pressure of a liquid equals the pressure around the liquid and the liquid transforms into a vapour. The boiling point of a liquid is affected by the surrounding atmospheric pressure. The boiling point of a liquid in a partial vacuum is lower than the boiling point of the same liquid at atmospheric pressure. The boiling point of a liquid at high pressure is greater than the boiling point of the same liquid at atmospheric pressure.

Complete answer:
Salt, or sodium chloride, is an ionic substance with the chemical formula 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.
There are no distinct sodium chloride molecules in solid sodium chloride. Every sodium ion in the lattice is electrostatically linked to every other chloride ion. Of course, every other sodium ion repels it electrostatically, but if you add up all of these interactions, which is absolutely possible, the net electrostatic interaction is favourable. Because of the strong electrostatic interaction between its positive and negative ions, sodium chloride has a high melting and boiling point. This needs greater heat energy to overcome the force of attraction. Given this non-molecular structure, we should expect high melting and boiling temperatures, which we do.
When you dissolve salt in water, sodium and chloride ions are formed. The ions would recombine to produce solid salt if all the water was removed from the boil. Boiling the NaCl, on the other hand, poses no risk: Sodium chloride has a boiling point of 2575 degrees Fahrenheit (1413 degrees Celsius). The boiling point of salt, like that of other ionic solids, is exceptionally high.

Note:
Water molecules can form ion-dipole interactions with individual sodium and chloride ions now that sodium chloride is soluble to some extent in water. The dissolution is somewhat endothermic, which means that the ion-dipole bonds formed between the ions and the solvent molecules nearly perfectly balance the lattice enthalpy of sodium chloride.