Question

o most soluble) Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble) LiF < NaNO3 < CHCl3 CH3OH < CH4 < LiF CH4 < NaNO3 < CHCl3 CCl4 < CHCl3 < NaNO3 CH3OH < Cl4 < CHCl3

Answer 1

Answer: Option (d) is the correct answer.

Explanation:

As it is known that like dissolves like. So, water being a polar compound is able to dissolve only polar compounds.

Hence, a compound that is ionic or polar in nature will readily dissolve in water. Whereas non-polar compounds will be insoluble in water.

As $CCl_{4}$ is a non-polar compound. Hence, it is insoluble in water.

On the other hand, $CHCl_{3}$ is a polar compound due to difference in electronegativity of chlorine and carbon atom there will be development of partial charges. Hence, there will be dipole-dipole forces existing between them.

Whereas $NaNO_{3}$ is an ionic compound and it will readily dissociate into ions when dissolved in water. Also, there will be ion-dipole interactions between sodium and nitrate ions.

Hence, $NaNO_{3}$ will readily dissolve in water.

Thus, we can conclude that the compounds correctly arranged in order of increasing solubility in water are $CCl_{4}$ < $CHCl_{3}$ < $NaNO_{3}$.