1. Dissolution: The solid particles break down into individual ions or molecules and become surrounded by water molecules. This process is called dissolution. The water molecules form a hydration shell around the ions or molecules, which helps to separate them from each other and keep them dissolved.
2. Formation of a solution: The dissolved solid particles are now evenly distributed throughout the water, forming a homogeneous mixture called a solution. The water is the solvent and the dissolved solid is the solute.
3. Dynamic equilibrium: The dissolution process is often a reversible reaction. This means that some of the dissolved solid particles can also re-crystallize and return to the solid state. The rate of dissolution and crystallization reach a balance, leading to a dynamic equilibrium.
Factors influencing solubility:
* Temperature: Solubility of most solids increases with temperature.
* Pressure: Pressure has little effect on the solubility of solids.
* Nature of solute and solvent: The polarity of the solute and solvent play a significant role in solubility. "Like dissolves like" - polar solutes dissolve in polar solvents, and non-polar solutes dissolve in non-polar solvents.
Examples of soluble solids:
* Sugar
* Salt
* Baking soda
* Potassium permanganate
Note: Some solids are only slightly soluble in water, while others are highly soluble. The extent of solubility depends on the specific solid and the conditions.
