The opposing charges of Li+ and Cl-ions cause the solvent molecules to round the ions when LiCl is introduced to the polar solvent CH3COCH3. The partial positive and negative charges on the polar solvent molecules draw ions and aid in the dissolution of the ionic bonds in LiCl. Consequently, the solvent molecules encircle and separate the Li+ and Cl-ions, thereby dissolving the LiCl in CH3COCH3.
The process of dissolving LiCl in CH3COCH3 can be represented by the following chemical equation:
LiCl(s) + CH3COCH3(l) → Li+(aq) + Cl-(aq) + CH3COCH3(l)
In this equation, the solid LiCl dissociates into its constituent ions (Li+ and Cl-) when introduced to the polar solvent CH3COCH3. The solvent molecules surround and solvate the ions, effectively breaking the ionic bonds in LiCl and allowing it to dissolve.
Overall, the ability of polar solvents like CH3COCH3 to dissolve ionic compounds such as LiCl is a result of the electrostatic interactions between the ions and the partial charges on the solvent molecules. This process is essential for the formation of solutions and plays a crucial role in various chemical reactions and processes.