Final answer:
To determine the final temperature of a solution, assess the heat of solution, calculate the molar concentration, and understand the effect of temperature on solubility. An increase in temperature upon dissolution suggests an exothermic process, while solubility can vary with temperature, following Henry's Law for gases.
Step-by-step explanation:
To determine the final temperature of a saturated solution of LiF(s) in water and the heat of solution, you need to consider the initial and final temperatures, the quantity of LiF added, the mass of water, and the specific heat capacity of water (if it is not significantly different from the solution). The dissolution of a solute in a solvent can be either exothermic (releasing heat) or endothermic (absorbing heat), leading to a change in the solution's temperature.
For example: when a solute dissolves and the temperature of the solution rises, as described with CaCl₂, it indicates that the dissolution process was exothermic.
To find the molar concentration of a saturated solution, you could use the solute's mass and the volume of the solution. This enables the calculation of the solubility in moles per liter (molarity).
In regards to the effect of temperature on solubility, as the temperature increases, the solubility of gases in liquids generally decreases (according to Henry's Law), while the solubility of many solids increases.
As an exercise, we can calculate the temperature change during dissolution by noting the initial and final temperatures of a substance when it is added to a solvent. For instance, if the initial temperature is 23.0°C and the final temperature after dissolution is 34.7°C, the change in temperature is +11.7°C. This indicates that the dissolution was likely endothermic, as heat was absorbed to raise the temperature.