On the heat of solution of sodium hydroxide in water
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I’m not very familiar with chemical engineering, and I’d like to ask a question: assuming the temperature of pure water is 20°C, when sodium hydroxide is added to the water, as the mass of the solute increases, heat of solution is released and the temperature of the solution rises. I’ve come up with a method for extracting the solute, sodium hydroxide: by lowering the temperature of the solution. As the temperature drops until saturation, will sodium hydroxide precipitate if the temperature is lowered further? Or some other substance. Are there other methods to extract sodium hydroxide?
What is the concentration of sodium hydroxide in the original solution from which you want to extract it? What you mean by extracting sodium hydroxide by cooling refers to the method of reducing solubility by lowering the temperature; one of the prerequisites for this method to work is that your original solution must contain sufficient amounts of sodium hydroxide. To determine whether it’s feasible or not, go and check the specific solubility of sodium hydroxide first.
I found a chlorine-alkali manual that is quite comprehensive; thank you
What do you want to do? Do you think that a little bit of knowledge obtained from someone who is completely inexperienced is what you want, and that you can understand and apply it even if what that person says contains inaccuracies? Either go and read the Chlor-Alkali Manual Systematics*, or post the original question as it is – don’t try to interpret it with your unreliable understanding