The solubility of potassium chloride KCl in water at 25C is approximately 34 grams per 100 grams of water. This means that at 25C, you can dissolve 34 grams of KCl in 100 grams of water to form a saturated solution.The solubility of KCl in water increases with increasing temperature. For example, at 0C, the solubility is about 28 grams per 100 grams of water, while at 100C, it is about 56 grams per 100 grams of water. This trend is common for most ionic compounds.The conceptual explanation for this behavior is based on the principles of solvation and intermolecular forces. When KCl is dissolved in water, the ionic bonds between the potassium K+ and chloride Cl- ions are broken, and the ions become surrounded by water molecules. This process is called solvation. The negatively charged oxygen atoms in the water molecules are attracted to the positively charged K+ ions, while the positively charged hydrogen atoms in the water molecules are attracted to the negatively charged Cl- ions. These attractive forces between the ions and water molecules are called ion-dipole interactions.The solvation process is endothermic, meaning it requires energy to break the ionic bonds in KCl and form new ion-dipole interactions between the ions and water molecules. As the temperature of the water increases, more thermal energy is available to overcome the energy barrier required for solvation. Consequently, more KCl can dissolve in the water, leading to an increase in solubility with increasing temperature.In summary, the solubility of potassium chloride KCl in water at 25C is approximately 34 grams per 100 grams of water, and the solubility increases with increasing temperature. This behavior can be explained by the endothermic nature of the solvation process and the increased availability of thermal energy to overcome the energy barrier required for solvation at higher temperatures.