The correct order of the solubility of alkaline-earth metal...

The correct order of the solubility of alkaline-earth metal sulphates in water is : (a) $\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}$ (b) $\mathrm{Mg}>\mathrm{Sr}>\mathrm{Ca}>\mathrm{Ba}$ (c) $\mathrm{Mg}<\mathrm{Ca}<\mathrm{Sr}<\mathrm{Ba}$ (d) $\mathrm{Mg}<\mathrm{Sr}<\mathrm{Ca}<\mathrm{Ba}$

The correct order of the solubility of alkaline-earth metal sulphates in water is :
(a) $\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}$
(b) $\mathrm{Mg}>\mathrm{Sr}>\mathrm{Ca}>\mathrm{Ba}$
(c) $\mathrm{Mg}<\mathrm{Ca}<\mathrm{Sr}<\mathrm{Ba}$
(d) $\mathrm{Mg}<\mathrm{Sr}<\mathrm{Ca}<\mathrm{Ba}$

Key Concepts

Sulfate Ion

The sulfate ion (SO4²?) is a polyatomic ion with a tetrahedral arrangement of oxygen atoms around a central sulfur atom. Its charge and structure impact the properties of the salts it forms with metal cations, including factors that influence solubility in aqueous solutions.

Solubility

Solubility is the ability of a substance (solute) to dissolve in a solvent, forming a homogeneous mixture. It depends on the interactions between the solute and solvent particles and is influenced by factors such as temperature, pressure, and the nature of the chemical species involved.

Lattice Energy

Lattice energy is the energy released when oppositely charged ions in the gaseous state come together to form an ionic solid. It also represents the energy required to break apart the ionic solid into its individual ions. High lattice energy implies strong ion–ion interactions, which can reduce a compound's solubility.

Hydration Energy

Hydration energy is the energy released when ions are surrounded and stabilized by water molecules during the dissolution process. It helps to overcome the lattice energy of ionic compounds. When hydration energy exceeds lattice energy, the compound is more likely to dissolve.

Trends in Solubility of Ionic Compounds

The solubility of ionic compounds is generally determined by the balance between lattice energy and hydration energy. Variations in ionic size, charge density, and structure can lead to predictable trends in solubility, which are essential for understanding how changes across a group in the periodic table affect the dissolution of different salts.

Alkaline-earth Metals

Alkaline-earth metals, located in Group 2 of the periodic table, form +2 cations. Variations in their ionic radii and charge densities influence properties such as lattice and hydration energies of their compounds, ultimately affecting their solubility in water.

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