Why the solubility of alkaline earth metal hydroxides increases down the group while that of alkali metal sulphates decreases down the group?

Since lattice enthalpy decreases much more than the hydration enthalpy with increasing ionic size, the solubility increases down the group (↓). Since the hydration enthalpy decreases down the group, solubility will decreases as found for alkaline earth metal carbonates and sulphates.

Why does solubility of sulfates decrease down the group?

For sulphates: Solubility decreases as you go down the group. The lattice dissociation enthalpy and hydration enthalpy both decrease as you go down the group. The hydration enthalpy decreases more than the lattice dissociation enthalpy. Therefore the enthalpy of solution becomes more endothermic (or less exothermic).

How does the solubility of sulphates of alkaline earth metals vary down the group?

“Solubility of sulphates and carbonates of alkaline earth metals decreases as the atomic number of the metal increases down the group.”

Why solubility of alkali metals decreases down the group?

On moving down the group, their solubility further decreases because their lattice energy remains constant but hydration energy decreases and hydration energy becomes lower than lattice energy. Assertion :Statement-I: Solubilities of alkali metal fluorides and carbonates increase down the group.

Why does solubility increase down a group?

Group II metal hydroxides become more soluble in water as you go down the column. This trend can be explained by the decrease in the lattice energy of the hydroxide salt and by the increase in the coordination number of the metal ion as you go down the column.

Does solubility decrease down the group?

On going down the group, the size of the cation increases and the salt becomes more ionic in nature. So, the solubility also increases down the group.

Why solubility of sulphates of alkaline earth metals decrease down the group mainly due to decrease in?

The solubility of the sulphates of alkaline earth metals decreases down the group. It is because the hydration energy decreases down the group, the solubility of sulphates is also decreased down the group.

What happens to the solubility of the alkaline earth metals as you go down the periodic table ie what is the periodic trend for solubility )?

The periodic trend in the solubility of alkaline earth metal compounds is that as one goes down a group, it increases in activity. Therefore, the unknown alkaline earth compound in Part B is strontium chloride (SrCl2).

Why the solution of alkali metals in liquid ammonia are Coloured?

Alkali metals dissolve in liquid ammonia giving deep blue solutions, which conduct electricity. The blue colour of the solution is due to ammoniated electrons, which absorb energy in the visible region of light.

How does the solubility of alkaline earth metals change down the group?

The ability of alkaline earth metal cations to hydrate themselves decreases down the group due to decrease in charge density. As the hydration enthalpy decreases on going down the group, the solubility of the carbonates and sulphates also decreases.

Why does the solubility of carbonates and sulphates decrease down the group?

Thus the solubility increases. The reason for the decrease of solubility of their carbonates and sulphates decreases down the group because of the following reason. The hydration enthalpy decreases due to the continuous increase in the size of cation down the group.

Which of the following is the least soluble alkaline earth metal ion?

Beryllium ion is the most soluble and the solubility decreases with increasing size so that Barium ion is the least water-soluble alkaline earth metal ion. Solubility in water is related to the ionic nature and size. Smaller ions have higher charge density and can be solvated by more water molecules.

How does the solubility of a compound change down the group?

Thus the solubility increases. The hydration enthalpy decreases due to the continuous increase in the size of cation down the group. In simple words, the energy released during the dissolution of a solute in water due to the formation of new bonds between them decreases.