Regarding the issue of the boiling point elevation of solutions
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For a certain solution, its boiling point is related to the concentration of the solution. At normal pressure, the boiling point of a sodium nitrate solution with a concentration of (150 g/100 g H2O) is 115°C, while the boiling point of a sodium nitrate solution with a concentration of (180 g/100 g H2O) is 117°C. I have a question: At atmospheric pressure, a sodium nitrate solution with a concentration of (150 g/100 g H2O) starts to boil at a temperature of 115°C. As the water solvent evaporates, the solution becomes more concentrated, and its boiling point rises above 115°C; at this point, the solution stops boiling. So how can continuous evaporation of the solution be achieved in an evaporator?
The utility heating system you use must be capable of temperatures higher than 115°C, so the temperature inside the evaporator also increases gradually.
Where can I find the boiling point of a sodium nitrate solution?
The boiling point changes even under slight pressure; so if a certain pressure range is maintained, continuous evaporation can be achieved, right?