Which of the following substances are likely to be soluble...

Which of the following substances are likely to be soluble in water?
(a) $\mathrm{Ag}_{2} \mathrm{O} \quad$ (b) $\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\quad$ (c) $\mathrm{SnCO}_{3} \quad$ (d) $\mathrm{Fe}_{2} \mathrm{O}_{3}$

Key Concepts

Solubility Rules

Solubility rules are generalized guidelines used to predict whether a given chemical compound will dissolve in water. These rules are based on the types of ions present and their interactions with water molecules. For example, nitrates and most alkali metal salts are generally soluble, while many transition metal oxides and carbonates show limited water solubility.

Ionic Compounds

Ionic compounds consist of positively and negatively charged ions held together by strong electrostatic forces. When they dissolve in water, these compounds dissociate into their individual ions. The process is facilitated by the polar nature of water, which stabilizes the ions through ion–dipole interactions.

Polar Solvents

Water is a polar solvent, meaning it has a positive and a negative end due to its molecular geometry and electronegativity differences. This polarity allows water molecules to surround and interact with charged particles or polar molecules, aiding in the dissolution of ionic compounds and certain polar covalent compounds.

Metal Oxide Chemistry

The solubility of metal oxides in water can vary greatly; some metal oxides react with water to form hydroxides, while others remain insoluble due to strong ionic lattices or thermodynamic stability. The solubility of a metal oxide is often influenced by the charge density of the metal ion and the structure of the oxide.

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