A saturated solution of kcl is prepared at 25degree celsius. What would happen if temperature is cooled to 10degree celcius? ????????
When a saturated solution of KCl is prepared at 25 degrees Celsius and then cooled to 10 degrees Celsius, a phenomenon known as temperature-driven solubility occurs.
First, let's understand the concept of solubility. Solubility refers to the maximum amount of solute (in this case, KCl) that can dissolve in a specific amount of solvent (usually water) at a given temperature. Saturated solutions are solutions in which the maximum amount of solute has been dissolved at a specific temperature.
In general, the solubility of most solids in water tends to increase with an increase in temperature. This means that as the temperature rises, more solute can dissolve in the solvent until the maximum solubility is reached, creating a saturated solution.
Now, when the saturated solution of KCl at 25 degrees Celsius is cooled to 10 degrees Celsius, the solubility of KCl in water decreases. This is because the solubility of KCl generally follows the trend that solubility decreases with a decrease in temperature.
As a result, the excess KCl in the solution will no longer be able to remain dissolved and will start to crystallize out of the solution. This means that you will observe the formation of visible crystals of KCl in the solution as it cools.
In summary, when a saturated solution of KCl prepared at 25 degrees Celsius is cooled to 10 degrees Celsius, the solubility of KCl decreases, leading to the formation of crystals as the excess KCl comes out of the solution.