At saturation temperature, how are all gases present in the solution?

At saturation temperature, gases present in a solution exist in free form. This is based on the understanding of how gases behave under varying pressures and temperatures. At saturation, the vapor pressure of the gas above the liquid is equal to the partial pressure of the gas in the liquid. This equilibrium means that the gas molecules have enough energy to escape the liquid phase and enter the vapor phase, indicating they are in a free form.

In a saturated solution, the gas is no longer being actively absorbed into the liquid but is instead present at a state of equilibrium. If additional gas is introduced or if the pressure changes, the system can adjust, which further supports the notion that the gas exists freely rather than being in a bound state, dissolved, or suspended.

The other forms listed, such as dissolved, suspended, or bound, suggest interactions or constraints that would prevent the gas from achieving a free, unbound state, which is contradictory to the very definition of saturation where the gas is allowed to exist in a gaseous state at the given temperature.