Of the following substances, which ones are generally...

Of the following substances, which ones are generally soluble in water? (See Figure $14.2$ or Appendix V.)
(a) $\mathrm{AgCl}$
(d) $\mathrm{NaOH}$
(b) $\mathrm{K}_{2} \mathrm{SO}_{4}$
(e) $\mathrm{PbI}_{2}$
(c) $\mathrm{Na}_{3} \mathrm{PO}_{4}$
(f) $\mathrm{SnCO}_{3}$

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Key Concepts

General Solubility Rules

These are empirical guidelines that predict the aqueous solubility of ionic compounds. They indicate that many salts containing alkali metal ions and the ammonium ion are soluble, while compounds with certain anions like chloride, sulfate, or phosphate may be insoluble except when paired with ions that form exceptions. These rules help in quickly determining whether a compound will dissolve in water.

Ionic Bonding and Lattice Energy

Ionic compounds are composed of positively and negatively charged ions held together by strong electrostatic forces in a crystal lattice. The energy required to break this lattice (lattice energy) must be overcome by the energy released when water molecules hydrate the ions (hydration energy) for the compound to dissolve. The relative magnitudes of these energies determine solubility.

Water as a Polar Solvent

Water is a highly polar molecule, meaning it has a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. This polarity enables water to stabilize ions by surrounding them with a solvation shell, thereby promoting the dissolution of substances that can separate into ions.

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