Saturation temperature is defined as the temperature at which a pure substance say water, changes phase, at a fixed pressure. So water boils at 100⁰C , if the external pressure is kept constant at 101.3 kPa(1atm). At 12.35 kPa water boils at 50°C, which indicates that there is a pressure-temperature dependence at saturation points, but is this p-t dependence driven by pressure only? i.e can we keep the pressure fixed at 1atm and still boil water at a temperature other than 100°C, by increasing the heat supply and hence increasing temperature.
Also, is this pressure-temperature dependence a consequence of the gibbs-phase rule.