NEET JEE MCQ/ Hydration Energy/Solubility of metal carbonates sulphates/Lattice energy/ BEST TRICK

Compare the solubility and thermal stability of the following compounds of the alkali metals with those of the alkaline earth metals. (a) Nitrates, (b) Carbonates, (c) Sulphates.
(i) Solubility
Nitrates, carbonates and sulphates of alkali metals are water soluble. On moving down the group, the solubility increases. This is because their lattice energies decreases more rapidly than their hydration energies.
Alkaline earth metal nitrates are water soluble. On moving down the group, their solubility decreases. This is because their hydration energies decreases more rapidly than their lattice energies.
Alkaline earth metal carbonates and sulphates have lower solubility than alkali metal carbonates and sulphates. The solubility of alkaline metal carbonates and sulphates decreases with decrease in hydration energy as we move down the group.
Compare the solubility and thermal stability of alkali metals carbonates with those of the alkaline earth metals nitrates.
Thermal stability ofAlkaline earth metal nitrate ---Alkaline earth metal nitrate decompose on heating.All alkaline earth metals Nitrates decompose to form metal oxide, NO 2 and O 2.
Thermal stability of alkali metal carbonate---- alkali metals carbonates are stable and do not decompose even at high temperature.
solubility of alkaline earth metal nitrates --Nitrates, of alkaline earth metals are soluble in water. thier solubility, however decreases as we move down the group because their hydration energies decreases more rapidly than the lattice energies.
Solubility of alkali metal carbonates ----alkali metals carbonates are soluble in water. Their solubility however increases as we move down the group since the lattice energies decreases more rapidly than the hydration energies.
Question
The hydroxides and carbonates of sodium and potassium are easily soluble in water while the corresponding salts of magnesium and calcium are sparingly soluble in water. Explain.
Lattice energy
The amount of energy required to convert one mole of an ionic solid into gaseous ionic constituents
Or
The amount of energy released when one mole of ionic solid is formed from its gaseous ionic constituents.
Hydration energy
Hydration energy is the amount of energy released on the hydration of a one-mole ion. When the solvent is not water it is known as solvation energy.
Condition for a substance to become soluble
The solubility of a compound in water depends on the balance between lattice energy and hydration energy. When hydration energy of any ion overcomes the amount of lattice energy the bond dissociates, and solubility occurs.
Explanation
The atomic size of sodium and potassium is larger than that of magnesium and calcium and the charge on
. Thus, the lattice energies of carbonates and hydroxides formed by calcium and magnesium are much more than those of sodium and potassium.
Also, we know if the size of cation and anion decreases, solubility increases because hydration energy increases.
In the case of hydroxides and carbonates of sodium and potassium get dissociated into the water and get solubilized because their hydration energy is greater than that of lattice energy while the hydroxides and carbonates of magnesium and calcium are sparingly soluble in water because their hydration energy is less than that of lattice energy.

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