Regarding the issue of sodium sulfite generated by desulfurization
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I’m seeking advice from experts: After incinerating waste liquids, the exhaust gases contain sulfur dioxide. When using wet desulfurization, is sodium sulfite the main substance that is removed? Can sodium sulfite be converted into sodium sulfate for recovery? Or how should the lotion be handled? Can it be treated through biochemical methods? Or emission?
If the purity of your sodium sulfite product is high, it can be sold as a commodity, whereas sodium sulfate has a very low price and thus poor economic viability. Why is your desulfurization by-product sodium sulfite? Is caustic soda or soda ash being used as the absorbent? These materials are expensive and costly; it’s better to use lime or limestone for treatment, as it is less costly.
When using an alkali solution for absorption, isn’t what is absorbed sodium sulfite? Is it sodium sulfate that is being produced? If dry desulfurization is used, the desulfurization efficiency is low, and it’s not possible to ensure that the exhaust gases emitted meet the required standards
What’s meant upstairs is that sodium sulfate isn’t valuable, so there’s no need to convert it into sodium sulfate for recycling. Using lime means that if recycling is not desired, lime can be used as an alkaline agent for absorption, and it is inexpensive.
I didn’t quite understand what the original poster meant. Using a Na-based desulfurizer sounds like the double-alkali method. This process uses Na2CO3 or NaOH as absorbents, which react with SO2 to produce Na2SO3. After the reaction, the slurry is discharged from the tower where it reacts with Ca(OH)2 to regenerate the sodium alkali; the reaction is as follows: Ca(OH)2 + Na2SO3 + H2O → 2NaOH + CaSO3·H2O. The regenerated NaOH slurry is returned to the tower for further use. In this process, the actual Ca salt that is consumed. Under oxidative conditions, CaSO3 can be further oxidized to form CaSO4. After that, it’s the usual gypsum dehydration process. In the early days, the inhibition of oxidation was used; the resulting sulfite solution was difficult to dehydrate. In power plants, it could be discharged together with boiler ash.
This post was last edited by Refinery Operator on 2011-4-13 22:07. Does anyone have sodium sulfite produced by the sodium-alkali method for sale? A sodium sulfite content of 20% (for liquid) or 60% (for solid) or higher is sufficient
The original poster can check out the environmental protection section to learn about the sodium-alkali method for desulfurization. After sodium hydroxide absorbs SO2, the product is sodium sulfite, which has high economic value and can be sold as a commodity.