Final Answer:
The compounds that would behave similarly to KCl in water, forming a solution able to conduct electricity, are LiCl and SrCl2. Options D and C are answers.
Step-by-step explanation:
The ability of a compound to dissolve in water and form a conductive solution depends on its ability to dissociate into ions. When an ionic compound dissolves in water, the positive and negative ions are surrounded by water molecules, forming a solution that conducts electricity.
a) PbCl2: PbCl2 is a sparingly soluble ionic compound. It does not dissociate completely in water, meaning it does not form a significant number of ions in solution. Therefore, it does not conduct electricity well.
b) LiK: LiK is not an ionic compound. It is a salt containing the lithium cation (Li+) and the potassium cation (K+). These cations exist as free ions in the solid state and do not need to dissociate in water. Therefore, LiK is already conductive and does not require dissolving in water for this property.
c) LiCl: LiCl is a highly soluble ionic compound. It dissociates completely in water, forming a high concentration of Li+ and Cl- ions. This solution readily conducts electricity.
d) SrCl2: SrCl2 is a soluble ionic compound. It dissociates readily in water, forming a sufficient concentration of Sr2+ and Cl- ions. This solution also conducts electricity well.
Therefore, LiCl and SrCl2 are similar to KCl in their ability to dissolve in water and form conductive solutions due to complete dissociation into ions.
Options D and C are answers.