When dealing with the behavior of gases and liquids under pressure, it is important to refer to principles derived from the ideal gas laws and the concept of incompressibility for liquids. In this instance, the situation is analyzed using Boyle's Law, which states that for a given amount of gas at constant temperature, the volume of the gas is inversely proportional to its pressure.
However, liquids are often considered incompressible, meaning that their volume does not change significantly when pressure is applied. If the temperature of the liquid remains constant and the pressure is tripled, the volume of the liquid does not contract appreciably because the molecules are already closely packed together and don’t have significant space to reduce volume under increased pressure. Thus, the volume remains effectively the same despite the increase in pressure.
This principle helps clarify why an increase in pressure does not lead to any significant change in the volume of the confined liquid, reaffirming that it stays constant under these conditions.