Separation problem of potassium chloride and sodium sulfate
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This post was last edited by sunjl1981 on 2013-1-7 00:24. There is currently a stream of water containing 7% KCl and 5% Na2SO4. I don't know any good way to separate it. Please help me. This post was last edited by yzhms on 2009-4-11 15:42 ] # hcbbs
First (multiple effects) evaporate and concentrate the material liquid to a certain extent, and then do cooling (freezing) crystallization. The hydrate of sodium sulfate should precipitate first. I remember that for aqueous solutions containing sodium chloride and sodium sulfate, as long as the concentration of sodium chloride is less than 18%, sodium sulfate hydrate will be crystallized by cooling. If the concentration of sodium chloride is higher, the first thing to crystallize is mixed salt.
I would like to ask, what is the purpose of separation? Is it just Na2SO4 or NaCl or both? This post was last edited by yzhms on 2009-4-11 15:42 ]
What they are talking about is potassium chloride. This wastewater may produce potassium glauberite. It can be evaporated to saturation temperature first, and then cooled to about 25 degrees to generate potassium mirabilite, which can then be re-dissolved and crystallized, and sodium chloride can be thermally separated. Finally, potassium sulfate can be obtained, which is a good resource.
“After cooling to about 25 degrees, potassium mirabilite can be generated and then redissolved and crystallized, and sodium chloride can be thermally separated. Finally, potassium sulfate can be obtained, which is a good resource." Potassium sulfate has a small solubility and is greatly affected by temperature. Should it be recrystallized by cold method? “"Thermal precipitation of sodium chloride", how to do it?
The evaporation concentration method is subject to discussion! because: 1. Depending on the concentration, the energy consumption is higher. ； 2. To cool and separate, you must also look at the phase diagram rules. Personally, I feel that potassium sulfate and its double salt may precipitate if cooled. ； It is recommended to freeze directly in the freezer at -5°C, as most of the sodium sulfate may precipitate out. ； However, energy consumption issues must also be taken into consideration. Personally, I feel that recycling is of little significance! For reference only!
In addition, if there is a salt factory nearby, you can consider discharging it into the salt farm and integrating it into the production system of the salt factory, which can solve the problem.； Or add calcium chloride to the solution, and then perform sedimentation, separation, and evaporation cooling. ；
I don’t know if the poster has recycled it and used it for desalination. If so, it is better to remove the salt directly and add barium chloride to the water. Even if it is used as potassium alkali, it will not increase the Nacl content too much. The amount of water is small after all. In this case, there is no need to separate it. Just add less and mix it in, haha;P
In addition to talking about theory, everyone also considers costs. Evaporation and crystallization are not the price of tofu in exchange for meat. I think there are economical ways to increase the added value of this waste liquid.
For this kind of question, please consult directly with the people at the Salt Lake Research Institute. They are very experienced in extracting potassium sulfate. In fact, it is to take potassium sulfate out of the solution through the conversion of different conditions. It seems simple, but in fact the design and operation of the process flow are very particular.
I don’t know how the poster’s equipment is running now. I’m facing a similar problem to the poster. I am separating sodium chloride and sodium sulfate. I wonder if the poster can briefly introduce the process of your equipment. Thank you.
Hello, we have the technology to separate sodium chloride and sodium sulfate. Welcome to communicate QQ627865433
I wonder if the poster can briefly introduce your technology?