Question

Given,$$KCl$$ easily dissolves in water because:
A) It is a salt of potassium
B) It reacts with water
C) It is an electrovalent compound
D) Its ions are easily solvated

Answer 1

Hint: We must have to remember that the $$KCl$$ is an ionic compound. It dissociates itself into potassium and chlorine. As we know , potassium chloride is characterized by a colorless, crystalline appearance and an odorless smell. In its solid form, potassium chloride can be easily dissolved in water and the resulting $$KCl$$ solution is said to have a salty taste.

Complete answer:
When we talk of salvation of ions we must know about the lattice energy and hydration energy. Lattice energy of $$KCl$$ is less than hydration energy of $$K^{+}C{l}^{-}$$.$$K^{+}$$and $$C{l}^{-}$$get surrounded by water molecules and these ions remain separate and dissolved in water. So, $$KCl$$ is easily soluble in water. We must know that the $$KCl$$ has a high tendency to dissociate into ions so as it is introduced into water it dissociates completely (almost) into ions and dissolves in it. Hence dissolves readily in polar solvents like water due to existence in the form of ions.
So the correct option for this question is option D, as potassium chloride ions get easily solvated. We must remember that in the solid-state, $$KCl$$ is readily soluble in many polar solvents, including water. The salt is ionized into the $$K^{+}$$ cation and the $$C{l}^{-}$$ anions in these polar solvents.

So the correct option for this question is option D.

Note:
We have to know that the potassium chloride is completely ionized into $$K^{+}$$ and $$C{l}^{-}$$ ions in water, the resulting aqueous solution exhibits high values of electrical conductivity. We need to remember that the reduction of potassium chloride into metallic can be achieved with the help of metallic sodium, despite the lower electropositivity of sodium when compared to potassium.