Saturated vapor pressure and boiling point pressure

The pressure of a gas when vaporization (evaporation) and liquefaction of a substance are in equilibrium at a certain temperature. The higher the saturated vapor pressure, the easier it is for the liquid to evaporate. The temperature at which a liquid mixture begins to boil under a certain pressure is called the boiling point at that pressure. The boiling point changes depending on the composition of the liquid. For pure compounds, the bubble point is the boiling point at a certain pressure. 　　It is the temperature at which the first bubble appears when a liquid of fixed composition is heated under constant pressure; in other words, it is the temperature at which such a liquid reaches vapor-liquid equilibrium with vapor at a given pressure. The bubble point varies with the liquid phase composition and pressure. When a minimum or maximum value appears in the relationship between the bubble point and the liquid phase composition, the temperature at which this extreme value occurs is referred to as the lowest boiling point or the highest boiling point, respectively. At these temperatures, the composition of the vapor phase is the same as that of the liquid phase, and such a mixture is called an azeotropic mixture. I searched on Baidu; in my opinion, if the pressure is not specified, it refers to normal pressure of 0.101325 MPa, while saturated vapor pressure is a property of a substance

Reply to 2# Under the Rainy Platanus Trees: It seems that the standard pressure has now been changed to 0.1 MPa