Give a detailed explanation of the oxoacid salts of alkaline earth metal elements.

(A) Salts of oxoacids: The alkaline earth metals form various salts of oxoacids,including: $(a)$ Carbonates,$(b)$ Sulphates,and $(c)$ Nitrates.
$(a)$ Carbonates: Carbonates of alkaline earth metals are insoluble in water and can be precipitated by adding sodium or ammonium carbonate to a solution of their soluble salts. The solubility of these carbonates in water decreases as the atomic number of the metal ion increases. All carbonates decompose on heating to yield carbon dioxide and the metal oxide. $BeCO_{3}$ is unstable and must be stored in an atmosphere of $CO_{2}$. Thermal stability increases with increasing cationic size.
$(b)$ Sulphates: The sulphates of alkaline earth metals are white solids and are stable to heat. $BeSO_{4}$ and $MgSO_{4}$ are readily soluble in water,while solubility decreases from $CaSO_{4}$ to $BaSO_{4}$. The high hydration enthalpies of $Be^{2+}$ and $Mg^{2+}$ ions overcome the lattice enthalpy,making their sulphates soluble.
$(c)$ Nitrates: Nitrates are prepared by dissolving carbonates in dilute nitric acid. $Mg(NO_{3})_{2}$ crystallizes with six molecules of water,whereas $Ba(NO_{3})_{2}$ crystallizes as an anhydrous salt. This reflects a decreasing tendency to form hydrates as the cationic size increases and hydration enthalpy decreases. All nitrates decompose on heating to form the corresponding oxide: $2 M(NO_{3})_{2} \rightarrow 2 MO + 4 NO_{2} + O_{2}$ (where $M = Be, Mg, Ca, Sr, Ba$).