Which of the following salts will be insoluble in water? Co(NO3)2, CsBrO4, CePO4, Cs3 AsO4, BaSe

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Which of the following salts will be insoluble in water?...

Which of the following salts will be insoluble in water? $\mathrm{Co}\left(\mathrm{NO}_3\right)_2, \mathrm{CsBrO}_4$, $\mathrm{CePO}_4, \mathrm{Cs}_3 \mathrm{AsO}_4, \mathrm{BaSeO}_4, \mathrm{Hg}_5\left(\mathrm{IO}_6\right)_2, \mathrm{TiO}_2$.

Key Concepts

Solubility Rules

Solubility rules are guidelines used to predict whether an ionic compound will dissolve in water. They generally state that salts containing nitrate, acetate, and alkali metals (like lithium, sodium, or cesium) are soluble, whereas many salts of transition metals and many phosphates, carbonates, and sulfates tend to be insoluble unless paired with alkali metals or ammonium ions.

Lattice Energy versus Hydration Energy

The solubility of a salt in water is influenced by the competition between lattice energy—the energy required to break apart the ionic lattice—and hydration energy—the energy released when water molecules surround and stabilize the ions. When the hydration energy is lower than the lattice energy, the salt is less likely to dissolve.

Role of Alkali Metals in Enhancing Solubility

Compounds containing alkali metal ions (such as cesium or sodium) are typically highly soluble in water because these ions have lower charge densities and form weaker ionic lattices. This makes it easier for water to interact with and separate the ions during dissolution.

Insolubility Trends for Phosphates, Selenates, and Metal Oxides

Many phosphate salts are insoluble except when combined with alkali metals or ammonium. Similarly, selenate compounds and certain transition metal oxides often display low solubility in water due to their high lattice energies and the formation of stable, often polymeric, structures that water molecules cannot easily disrupt.

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