The polar solvent, CH3COCH3, pulls apart the LiCl crystal lattice by attracting and surround the Li+ ions with its partial negative charges, while the Cl- ions are surrounded with the partial positive charges, causing the compound to dissolve.
When LiCl dissolves in a polar solvent such as CH3COCH3, the positive Li ions and negative Cl ions become surrounded by the solvent molecules due to their opposite charges, resulting in the separation and dispersion of the ions throughout the solvent.
The process by which the ionic compound LiCl would dissolve in the polar solvent CH3COCH3 involves the solvent molecules attracting the oppositely charged ions in LiCl, causing the ions to separate and become surrounded by solvent molecules, forming a solution. Now to answer this question, we need to understand how polar solvents interact with ionic compounds. Polar solvents have molecules with a positive and negative end or pole. When an ionic compound like LiCl is added to a polar solvent like CH3COCH3, the positive (Li+) ions are attracted to the negative pole of the solvent molecules, while the negative (Cl-) ions are attracted to the positive pole of the solvent molecules. This attraction between the ions and the solvent leads to the separation of the ions from the solid crystal of LiCl. The solvent molecules surround the separated ions, creating a solvation or hydration shell around them, which makes them soluble in the polar solvent. The resulting solution consists of the ions dispersed throughout the solvent.
