The saturation vapor pressure of a liquid depends on its temperature. When a liquid evaporates, it turns into a gas or vapor. This process of evaporation depends on the energy of the liquid molecules. The higher the temperature, the more energy the molecules have, and the more likely they are to escape from the surface of the liquid and become a gas.
As the concentration of vapor molecules increases above a liquid surface, some of them may condense back into the liquid phase, and this creates an equilibrium between the liquid and vapor phases, called saturation.
The saturation vapor pressure is the pressure exerted by the vapor in equilibrium with its liquid phase at a given temperature. So, as the temperature of the liquid increases, the saturation vapor pressure increases, meaning more molecules are in the gas phase. On the other hand, as the temperature decreases, the saturation vapor pressure decreases, indicating fewer molecules in the gas phase.
Therefore, the saturation vapor pressure of a liquid is determined by its temperature and is independent of the volume, mass, density, or pressure of the liquid.