Solubility Variation with Temperature

A chemist is investigating the solubility of compounds in water. The chemist notices that as the temperature of the water increases, the solubility of salt (NaCl) increases, while the solubility of a gas, such as carbon dioxide (CO2), decreases. Based on these observations, the chemist decides to conduct an experiment to quantify the changes in solubility with temperature variations.

In the experiment, the chemist prepares saturated solutions of both sodium chloride and carbon dioxide in water at different temperatures (25°C, 50°C, and 75°C) and measures the amount of each solute that dissolves at these temperatures. The solubility product constant (Ksp) for NaCl can be approximated as independent of temperature within this range, while the solubility of CO2 in water follows Henry's law, which states that the amount of gas that dissolves in a liquid is directly proportional to its partial pressure above the liquid.