1. Solubility equilibrium

2. Solubility
Property of a solid, liquid, or gaseous chemical substance (solute) to dissolve in a solid, liquid, or gaseous substance (solvent).
As a result homogenous mixture is created.

3. Solubility
Usually expressed as the maximum amount of a substance, which can be dissolved in a specific volume of the solvent, under defined pressure and temperature conditions.
In certain conditions metastable supersaturated solution can be created.

4. Solubility depends on the type of solute the type of solvent
temperature
pressure
common-ion effect
complexation
ionic strength
crystal size

5. Range
Various substances solubility can vary in wide range. Substances sometimes are known as "insoluble", "poorly soluble", "highly soluble". Nowadays chemicals often takes the solubilities in range from kg/kg to complete miscibility with the solvent.

6. Sparingly soluble electrolyte
When the sparingly soluble electrolyte is put in water, only a small part goes into solution.
The transition electrolyte molecules to the the liquid phase is called dissolution. It is associated with the molecules breakdown into ions: electrolytic dissociation.
Dissolution is often accompanied by the solvolysis and solvation processes .

7. Solvatation
Solvation is the process of surrounding solute with solvent.
Usually for highly polar solvents, especially when a soluble compound also has a strong polar properties or has ionic bonds. The solvation phenomenon is often a prelude to dissociation process.

8. Solvolysis
The chemical reaction between the chemical compound that is present in solution and the solvent
Solvolysis reactions are often assigned specific names derived from reactive solvent.
Water – hydrolysis, alcohol, - alcoholysis, acetic acid - acetolysis.

9. Scheme
The concentration of dissolved particles is in equilibrium with the solid at the bottom. In the same unit time, the amount of particles that pass into solution is equal to the amount of patricles that precipitated.

10. Equilibrium

11. Solubility product

12. Solutions
Where the product of the ion concentrations is higher than the solubility product solution is supersaturated.
Where the product of the ion concentrations is equal to the solubility product solution is saturated.
Where the product of the ion concentrations is lower than the solubility product solution is unsaturated.

13. Usage
Solubility product allows to calculate the concentration of saturated electrolyte solution

14. Example salt A2B3

15. Example salt A2B3

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17. Example 1
Solubility of calcium carbonate in water at a temperature of 25°C, is 5*10-9. What is the solubility of the salt, expressed in g/l under these conditions?

18. Example 1 solution

19. Example 1 solution

20. Example 2
Solubility product of silver sulfate (VI) in water, at a temperature 25°C is 7*10-5. What is the solubility of the salt, expressed in g/l under these conditions?

21. Example 2 solution

22. Example 2 solution

23. Example 3
The solubility of magnesium hydroxide at a temperature 180°C is equal to 2 × 104 mol/l. Find the solubility product of magnesium hydroxide.

24. Example 3 solution

25. Example 4
Lead iodide solubility product at room temperature is 1.4 * Calculate solubility of the salt at the same temperature and the concentration of Pb2+ and I- ion in the saturated solution.

26. Example 4 solution

27. Example 5
Equal volumes of 0.01M solutions of calcium chloride and sodium sulfate were mixed. Does the calcium sulfate precipitate forms? The solubility product of calcium sulphate is equal to 2.3 * 10-4.

28. Example 5 solution

29. Bibliography and other sources