Using solubility guidelines, predict whether each of the...

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: $(\mathbf{a}) \mathrm{MgBr}_{2,}$ $(\mathbf{b}) \mathrm{Pbl}_{2,}(\mathbf{c})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3},(\mathbf{a}) \mathrm{Sr}(\mathrm{OH})_{2},(\mathbf{e}) \mathrm{znSO}_{4}$

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water:
$(\mathbf{a}) \mathrm{MgBr}_{2,}$ $(\mathbf{b}) \mathrm{Pbl}_{2,}(\mathbf{c})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3},(\mathbf{a}) \mathrm{Sr}(\mathrm{OH})_{2},(\mathbf{e}) \mathrm{znSO}_{4}$

Key Concepts

Solubility Trends of Specific Anion Groups

Different anions follow distinct solubility trends. For example, bromides and iodides are generally soluble except when they form compounds with specific metal cations like lead or silver. Similarly, carbonates and hydroxides are typically insoluble unless they are paired with alkali metal ions or ammonium, whereas sulfates are mostly soluble but have exceptions with certain heavy cations.

Lattice Energy vs. Hydration Energy

The solubility of an ionic compound depends on the competition between lattice energy, which holds the ions together in a solid, and hydration energy, which stabilizes the ions when they are surrounded by water molecules. A compound is more likely to be soluble if the hydration energy exceeds the lattice energy.

General Solubility Guidelines

These are rules developed from empirical observations that help predict whether an ionic compound will dissolve in water. They include observations such as most salts containing alkali metal ions and the ammonium ion are soluble, nitrates and acetates are usually soluble, and certain anions like carbonates and hydroxides tend to be insoluble except when paired with the aforementioned cations.

Ionic Dissociation in Water

Ionic compounds dissolve in water by separating into their constituent cations and anions—a process known as dissociation. The extent of this dissociation is influenced by the interactions between the ions and water molecules.

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