Predict whether each compound is soluble in water. Indicate...

Predict whether each compound is soluble in water. Indicate which ions are present in solution for the watersoluble compounds.
(a) Potassium monohydrogen phosphate
(b) Sodium hypochlorite
(c) Magnesium chloride
(d) Calcium hydroxide
(e) Aluminum bromide

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Key Concepts

Solubility Rules

These are empirical guidelines used to predict whether an ionic compound will dissolve in water. They summarize patterns such as alkali metal salts and nitrates being generally soluble, while certain hydroxides, sulfides, and carbonates are often insoluble unless paired with specific cations. Understanding these rules is key to predicting the behavior of compounds in aqueous solution.

Dissociation of Ionic Compounds

When an ionic compound dissolves in water, it separates into its constituent ions—a process called dissociation. This concept is crucial for understanding how solid salts, upon interacting with water, break apart and allow individual ions to be surrounded and stabilized by water molecules.

Ion-Dipole Interactions

Ion-dipole interactions are the forces between the charged ions from the dissolved compound and the polar water molecules. These interactions help stabilize the ions in solution by orienting the water molecules around them, thereby overcoming the lattice energy of the ionic solid and facilitating its dissolution.

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