We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. (c) The hydrogen and oxygen bonds of water are easily broken by ionic solids.

Key Concepts

Ionic Compounds and Solubility

Ionic compounds consist of positively and negatively charged ions held together by strong electrostatic forces. When these compounds dissolve in water, the ionic bonds are overcome by the interactions with water molecules, allowing the ions to separate and disperse in solution. This process is essential for understanding how ionic solids behave in aqueous environments.

Polarity of Water

Water is a polar molecule, meaning it has a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. This polarity allows water molecules to interact effectively with charged ions, stabilizing them in solution through solvation. The ability of water to solvate ions is a key factor in its role as a solvent for ionic compounds.

Solvation Process

Solvation is the process by which solvent molecules surround and interact with solute ions or molecules. In the case of ionic solids dissolving in water, the water molecules surround the individual ions, effectively separating them from the solid lattice. This interaction is crucial for the dissolution of ionic compounds and is driven by the favorable energy changes associated with the formation of solute-solvent interactions.